Class 12 Chemistry Previous Year Questions, Chapter-wise (2022-2026)

Which of the following colligative properties can preferably determine the molar mass of proteins ?

1. Relative lowering of vapour pressure
2. Osmotic pressure
3. Elevation of boiling point
4. Depression of freezing point

For an electrolyte consisting of a monovalent cation and a monovalent anion undergoing dissociation in water, the van't Hoff factor (i) is :

1. less than 1
2. equal to 1
3. greater than 1
4. greater than 2

Which of the following solutions will have the lowest freezing point in water?

1. 0.1 M Glucose
2. 0.1 M CaCl2
3. 0.1 M KCl
4. 0.1 M Urea

Assertion (A): It is not possible to separate the components of an azeotrope by fractional distillation. Reason (R): Components of an azeotrope have the same composition in liquid and vapour phase and boil at a constant temperature.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following solutions will have the highest osmotic pressure?

1. 0.1 M KCl
2. 0.1 M CaCl2
3. 0.1 M Glucose
4. 0.1 M Urea

Assertion (A): Components of azeotropes are easily separated by fractional distillation. Reason (R): Components of an azeotrope have same composition in liquid and vapour phase.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A) : It is not possible to separate the components of an azeotrope by fractional distillation. Reason (R) : Minimum boiling azeotrope is formed by the solutions showing large positive deviation from Raoult's law.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The boiling point of an azeotropic mixture of water and ethanol is less than that of pure water and ethanol. The mixture shows:

1. positive deviation from Raoult's Law.
2. negative deviation from Raoult's Law.
3. no deviation from Raoult's Law.
4. that the solution is an ideal solution.

The mole fraction of a solute in 2·0 molal aqueous solution is:

1. 1·87
2. 0·347
3. 0·0347
4. 0·00347

The boiling point of an azeotropic mixture of water and nitric acid is more than that of pure water and nitric acid. The mixture shows :

1. no deviation from Raoult's law
2. that solution is an ideal solution
3. positive deviation from Raoult's law
4. negative deviation from Raoult's law

1 mole of liquid A and 2 moles of liquid B make a solution having a total vapour pressure 40 torr. The vapour pressure of pure A and pure B are 30 torr and 45 torr respectively. The above solution :

1. is an ideal solution.
2. shows negative deviation from Raoult's Law.
3. shows positive deviation from Raoult's Law.
4. is a maximum boiling azeotrope.

The boiling point of one molal NaCl solution, assuming NaCl to be completely dissociated in water is: (Kb for water = 0·52 K kg mol–1)

1. 100·52ºC
2. 101·04ºC
3. 100·04ºC
4. 101·52ºC

When a liquid and its vapour are at equilibrium and the pressure is suddenly decreased:

1. vapour pressure of the solution increases
2. heating occurs
3. cooling occurs
4. equilibrium remains unaffected

An azeotropic mixture of two liquids has a boiling point higher than that of either of the two liquids when it

1. obeys Raoult's law
2. shows positive deviation from Raoult's law
3. shows negative deviation from Raoult's law
4. obeys Henry's law

Solubility of gases in liquid decreases with increase in

1. pressure
2. volume
3. number of solute particles
4. temperature

The value of Henry's constant KH is:

1. greater for gases with higher solubility
2. greater for gases with lower solubility
3. constant for all gases
4. not related to the solubility of gases

Which of the following aqueous solutions will have the highest freezing point?

1. 1·0 M KCl
2. 1·0 M Na2SO4
3. 1·0 M Glucose
4. 1·0 M AlCl3

While doing qualitative analysis in chemistry lab, Abhishek added yellow coloured potassium chromate solution into a test tube. He was surprised to see the colour of the solution changing immediately to orange. He realised that the test tube was not clean and contained a few drops of some liquid. Which of the following substances will be the most likely liquid to be present in the test tube before adding potassium chromate solution?

1. Sodium hydrogen carbonate solution
2. Methyl orange solution
3. Sodium hydroxide solution
4. HCl solution

Assertion (A): Henry's law constant (KH) decreases with increase in temperature. Reason (R): As the temperature increases, solubility of gases in liquids decreases.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The freezing point of one molal KCl solution, assuming KCl to be completely dissociated in water, is : (Kf for water = 1·86 K kg mol–1)

1. – 3·72°C
2. + 3·72°C
3. – 1·86°C
4. + 2·72°C

A solution of acetone in ethanol :

1. obeys Raoult's law.
2. forms an ideal solution.
3. shows a positive deviation from Raoult's law.
4. shows a negative deviation from Raoult's law.

A solution of acetone in chloroform:

1. obeys Raoult's law.
2. forms azeotrope.
3. shows a positive deviation from Raoult's law.
4. shows a negative deviation from Raoult's law.

On mixing 30 mL of acetone with 20 mL of chloroform, the total volume of solution is:

1. equal to 10 mL
2. less than 50 mL
3. greater than 50 mL
4. equal to 50 mL

Which of the following solutions will have the highest boiling point in water ?

1. 1% KCl
2. 1% glucose
3. 1% urea
4. 1% CaCl2

Assertion (A): Cooking time is reduced in pressure cooker. Reason (R): Boiling point of water inside the pressure cooker is elevated.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following solution in water will have the lowest freezing point ?

1. 1% KCl
2. 1% glucose
3. 1% urea
4. 1% CaCl2

Assertion (A): Cooking time is reduced in pressure cooker. Reason (R): Boiling point of water inside the pressure cooker is lowered down.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following aqueous solutions will have the highest osmotic pressure?

1. 1% KCl
2. 1% glucose
3. 1% urea
4. 1% CaCl2

Assertion (A): Aquatic species are more comfortable in cold water than in warm water. Reason (R): Solubility of oxygen gas in water decreases with increase in temperature.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

For an electrolyte undergoing association in a solvent, the v factor:

1. is always greater than one
2. has negative value
3. has zero value
4. is always less than one

Assertion (A): When NaCl is added to water a depression in freezing point is observed. Reason (R): NaCl undergoes dissociation in water.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Phenol forms a dimer in benzene with a degree of association of 0.54. Its degree of association is:

1. 0.54
2. 0.46
3. 0.92
4. 0.27

Assertion (A): When NaCl is added in water, elevation in boiling point is observed. Reason (R): Elevation in boiling point is a colligative property.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

The system that forms maximum boiling azeotrope is:

1. CS2 and acetone
2. Benzene and toluene
3. Ethanol and acetone
4. Chloroform and acetone

Assertion (A): ΔHmix for an ideal solution is not equal to zero. Reason (R): A-B interactions in an ideal solution are same as between A-A and B-B interactions.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The relative lowering of vapour pressure of an aqueous solution containing non-volatile solute is 0·0225. The mole fraction of the non-volatile solute is:

1. 0·80
2. 0·725
3. 0·15
4. 0·0225

On mixing 10 mL of acetone with 50 mL of chloroform, the total volume of the solution will be:

1. < 60 mL
2. > 60 mL
3. = 60 mL
4. = 100 mL

A 1% solution is prepared by dissolving 1 g of sucrose (Molar mass = 342 g mol⁻¹) in 6 solution of the solute is :

1. 34·2 g mol⁻¹
2. 57 g mol⁻¹
3. 114 g mol⁻¹
4. 3·42 g mol⁻¹

Assertion (A): Addition of ethylene glycol to water lowers its freezing point. Reason (R): Ethylene glycol is insoluble in water due to lack of its ability to form hydrogen bonds with water molecules.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

A 1% solution of solute in 6 solution of sucrose (molar mass = 342 g mol-1). The molar mass of solute is:

1. 34·2 g mol-1
2. 57 g mol-1
3. 114 g mol-1
4. 3·42 g mol-1

Assertion (A): ΔmixH and ΔmixV are zero for non-ideal solutions. Reason (R): Solute-solvent interactions are not same as pure solute-solute and pure solvent-solvent interactions in non-ideal solutions.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

A solution is prepared by dissolving a 1% solution of sucrose (molar mass = 342 g mol⁻¹). The molar mass of the solute is:

1. 34.2 g mol⁻¹
2. 57 g mol⁻¹
3. 114 g mol⁻¹
4. 3.42 g mol⁻¹

Assertion (A): ΔHmix and ΔVmix are zero for an ideal solution. Reason (R): A solution which obeys Raoult's law over the entire range of concentration is called an ideal solution.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

The colligative property used for the determination of molar mass of polymers and proteins is:

1. Osmotic pressure
2. Depression in freezing point
3. Relative lowering in vapour pressure
4. Elevation in boiling point

Low concentration of oxygen in the blood and tissues of people living at high altitude is due to:

1. High atmospheric pressure
2. Low temperature
3. Low atmospheric pressure
4. Both low temperature and high atmospheric pressure

On dissolving ammonium chloride in water at room temperature, the solution feels cool to touch. Under which of the following conditions does salt dissolve faster?

1. Powdered salt in cold water
2. Powdered salt in hot water
3. Salt crystals in cold water
4. Salt crystals in hot water

Value of Henry's constant KH:

1. increases with decrease in temperature
2. decreases with increase in temperature
3. increases with increase in temperature
4. remains constant

Assertion (A): Osmotic pressure is a colligative property. Reason (R): Osmotic pressure is proportional to the molality.

1. Both (A) and (R) are true and (R) is the correct explanation of (A)
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A)
3. (A) is true, but (R) is false
4. (A) is false, but (R) is true

An azeotropic mixture of two liquids will have a boiling point lower than either of the two liquids when it

1. shows a negative deviation from Raoult's law
2. forms an ideal solution
3. shows a positive deviation from Raoult's law
4. is saturated

Assertion (A): Elevation in boiling point is a colligative property. Reason (R): The lowering of vapour pressure of solution causes elevation in boiling point.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3. (A) is true, but (R) is false.
4. (A) is false, but (R) is true.

Solubility of gas in liquid decreases with increase in

1. Pressure
2. Temperature
3. Volume
4. Number of solute molecules

Assertion (A): The enthalpy of mixing ΔHmix is equal to zero for an ideal solution. Reason (R): For an ideal solution the interaction between solute and solvent molecules is stronger than the interactions between solute-solute or solvent-solvent molecules.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3. (A) is true, but (R) is false.
4. (A) is false, but (R) is true.

Which of the following colligative property is used to find the molar mass of proteins?

1. Osmotic pressure
2. Elevation in boiling point
3. Depression in freezing point
4. Relative lowering of vapour pressure

Isotonic solutions have:

1. same osmotic pressure
2. same boiling point
3. same melting point
4. same vapour pressure

Kohlrausch gave the following relation for strong electrolyte: Λ = Λ° - A√C. Which of the following equality holds true?

1. Λ° = Λ as C → 0
2. Λ° = Λ as C → ∞
3. Λ = Λ° as C → 0
4. Λ = Λ° as C → 1

Which one of the following pairs will not form an ideal solution?

1. Benzene and Toluene
2. Nitric acid and Water
3. Hexane and Heptane
4. Ethyl chloride and Ethyl bromide

A compound undergoes complete tetramerization in a given organic solvent. Van't Hoff factor i is:

1. 40
2. 0.25
3. 0.125
4. 20

Assertion (A): When NaCl is added to water, a depression in freezing point is observed. Reason (R): The lowering of vapour pressure of a solution causes depression in the freezing point.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

A compound undergoes complete dimerization in a given organic solvent. The Van't Hoff factor is:

1. 20
2. 05
3. 025
4. 10

Assertion (A): When glucose is added to water, an elevation in boiling point is observed. Reason (R): The lowering of vapour pressure causes elevation in the boiling point.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

A compound CaCl2 . 6H2O undergoes complete dissociation in water. The van't Hoff factor is:

1. 9
2. 6
3. 3
4. 4

Assertion (A): When NaCl is added to water, a depression in freezing point is observed. Reason (R): The vapour pressure of solution is increased which causes depression in freezing point.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

1 mole of liquid A and 2 moles of liquid B make a solution having a total vapour pressure 40 torr. The vapour pressure of pure A and pure B are 45 torr and 30 torr respectively. The above solution

1. is an ideal solution
2. shows positive deviation
3. shows negative deviation
4. is a maximum boiling azeotrope

If molality of a dilute solution is doubled, the value of the molal elevation constant (Kb) will be

1. halved
2. doubled
3. tripled
4. unchanged

Which of the following aqueous solution will have highest boiling point?

1. 1.0 M KCl
2. 1.0 M K2SO4
3. 2.0 M KCl
4. 2.0 M K2SO4

The unit of molar conductivity is

1. S cm–2 mol–1
2. S cm2 mol–1
3. S–1 cm2 mol–1
4. S cm2 mol

Out of the following 1.0 M aqueous solutions, which one will show largest freezing point depression?

1. NaCl
2. Na2SO4
3. C6H12O6
4. Al2(SO4)3

State Raoult's law for a solution containing volatile components. Write any two characteristics of a solution which obeys Raoult's law at all concentrations.

What type of deviation from Raoult's law is shown by a mixture of phenol and aniline? Give reason. What will happen to the boiling point of the solution on mixing phenol and aniline?

What type of deviation from Raoult's law is shown by mixture of ethanol and acetone? Give reason. What will happen to the boiling point of the solution on mixing ethanol and acetone?

What type of deviation is shown by a mixture of chloroform and acetone from Raoult's law ? Give reason. What will happen to the boiling point of the solution on mixing chloroform and acetone ?

Explain why, on addition of 1 mol of KCl to 1 litre of water, the boiling point of water increases, while the addition of 1 mol of methyl alcohol to 1 litre of water decreases the boiling point.

(a) Explain the following with the help of Henry's law: (i) Bends (ii) Anoxia

(a) Explain the following with the help of Henry's law: (i) Bends (ii) Anoxia OR (b) How does sprinkling of salt help in clearing the snow covered roads in hilly areas? Write the name of the colligative property involved in this process.

(a) 1·00 molal aqueous solution of trichloroacetic acid is heated to its boiling point. Boiling point of this solution was found to be 100·18°C. Calculate the van't Hoff factor for trichloroacetic acid. (Given : Kb for water = 0·512 K kg mol⁻¹)

(a) 1·00 molal aqueous solution of trichloroacetic acid is heated to its boiling point. Boiling point of this solution was found to be 100·18°C. Calculate the van't Hoff factor for trichloroacetic acid. (Given: Kb for water = 0·512 K kg mol⁻¹) OR (b) State Henry's law. Calculate the mole fraction of CO2 in water at 298 K under 760 mm Hg. (Given: KH for CO2 in H2O at 298 K = 1·25 × 10⁶ mm Hg)

(a) Calculate the elevation of boiling point of a solution when 3 g of CaCl2 (Molar mass = 111 g mol–1) was dissolved in 260 g of water, assuming that CaCl2 undergoes complete dissociation. (Kb for water = 0·52 K kg mol–1)

State Henry's law. Why are aquatic species more comfortable in cold water as compared to warm water ?

State Raoult's law for a solution containing volatile components. Why is the vapour pressure of an aqueous solution of glucose lower than that of water?

Define osmotic pressure. Why is measurement of osmotic pressure method preferred for the determination of molar masses of macromolecules such as proteins and polymers?

What is meant by positive deviation from Raoult's law ? Give an example. What type of azeotrope is formed by positive deviation ?

What is meant by negative deviation from Raoult's law ? Give an example. What type of azeotrope is formed by negative deviation ?

(a) A and B liquids on mixing show rise in temperature. Which type of deviation from Raoult's law is there and why? (b) Why can azeotropic mixture not be separated by fractional distillation?

A 6% solution of glucose (molar mass = 180 g mol−1) is isotonic with 25% solution of an unknown organic substance. Calculate the molecular weight of the unknown organic substance.

A 4% solution of urea (molar mass = 60 g mol^-1) is isotonic with 52% solution of an unknown organic substance. Calculate the molecular weight of the unknown organic substance.

A 3% solution of glucose (molar mass = 180 g mol⁻¹) is isotonic with 25% solution of an unknown organic substance. Calculate the molecular weight of the unknown organic substance.

(a) Define molal depression constant. How is it related to enthalpy of fusion ?

Define molal depression constant. How is it related to enthalpy of fusion? OR What type of deviation is shown by ethanol and acetone mixture? Give reason. What type of azeotropic mixture is formed by that deviation?

A solution is prepared by dissolving 10 g of non-volatile solute in 200 g of water. It has a vapour pressure of 31.84 mm Hg at 308 K. Calculate the molar mass of the solute. (Vapour pressure of pure water at 308 K = 32 mm Hg)

The vapour pressure of pure liquid X and pure liquid Y at 25°C are 120 mm Hg and 160 mm Hg respectively. If equal moles of X and Y are mixed to form an ideal solution, calculate the vapour pressure of the solution.

Give reasons for the following: (a) Aquatic animals are more comfortable in cold water in comparison to warm water. (b) Sprinkling of salt helps in clearing the snow-covered roads in hilly areas.

On mixing liquid X and liquid Y, volume of the resulting solution decreases. The resulting solution shows what kind of deviation from Raoult's law? What change in temperature would you observe after mixing liquids X and Y?

How does the mixture of ethanol and acetone show deviation from Raoult's law? Give reason.

What is shown by a mixture of ethanol and acetone? Give reason.

Do ethanol and acetone form an azeotrope? Give reason.

Why is a mixture of ethanol and acetone unable to show the ideal behavior of Raoult's law? Give reason.

Calculate the molarity and molality of a KI solution if the density of 20% (mass/mass) aqueous solution of KI is 1·2 g mL−1. [Given : Molar mass of KI = 166 g mol−1]

Calculate the boiling point of a solution containing 0.61 g of benzoic acid (Molar mass = 122 g mol–1) in 5 g of CS2 in which it dimerises to the extent of 88%. The boiling point and Kb of CS2 are 46.2°C and 2.3 K kg mol–1 respectively.

When 1.5 g of a non-volatile solute was dissolved in 90 g of benzene, the boiling point of benzene got raised from 353.23 K to 353.93 K. Calculate the molar mass of the solute. (Given Kb for benzene = 2.52 K kg mol–1)

A solution containing 8.0 g of a non-volatile solute in 100 g of diethyl ether boils at 36.86 °C whereas pure diethyl ether boils at 35.60 °C. Determine the molar mass of the solute. (K b for diethyl ether = 2.02 K kg mol–1)

60 g of glucose is dissolved in 250 g of water. Calculate the freezing point of this solution. (molar mass of glucose = 180 g mol–1, Kf for water = 1.86 K kg mol–1)

An antifreeze solution is prepared by dissolving 31 g of ethylene glycol (Molar mass = 62 g mol^−1) in 600 g of water. Calculate the freezing point of the solution. (Kf for water = 1·86 K kg mol^−1)

Calculate the vapour pressure of a solution containing 61 g of benzoic acid (molar mass = 122 g mol–1) dissolved in 500 g of benzene when the vapour pressure of pure benzene at this temperature of experiment is 66 torr. Assume complete dimerization of benzoic acid in benzene.

An aqueous solution of NaOH was made and its molar mass from the measurement of osmotic pressure at 27°C was found to be 25 g mol–1. Calculate the percentage dissociation of NaOH in this solution. [Atomic mass: Na = 23 u, O = 16 u, H = 1 u]

An aqueous solution of NaOH was made and its molar mass from the measurement of osmotic pressure at 25°C was found to be 28 g mol⁻¹. Calculate the percentage dissociation of NaOH in this solution. [Atomic mass: Na = 23·0 u, O = 16·0 u, H = 1·0 u]

(a) Shweta mixed two liquids A and B of 10 mL each. After mixing, the volume of the solution was found to be 20·2 mL. (i) Why was there a volume change after mixing the liquids? (ii) Will there be an increase or decrease of temperature after mixing? (iii) Give one example for this type of solution.

Shweta mixed two liquids A and B of 10 mL each. After mixing, the volume of the solution was found to be 20·2 mL. Why was there a volume change after mixing the liquids ?

Vapour pressure of pure water at 298 K is 24·8 mm Hg. Calculate the lowering in vapour pressure of an aqueous solution which freezes at – 0·3°C. (Kf of water = 1·86 K kg mol–1)

03 g of acetic acid (Molar mass = 60 g mol–1) dissolved in 30 g of benzene shows a depression in freezing point equal to 0.45°C. Calculate the percentage association of acid if it forms a dimer in the solution. (Given : Kf for benzene = 5.12 K kg mol–1)

The vapour pressure of a solvent at 283 K is 100 mm Hg. Calculate the vapour pressure of a dilute solution containing 1 mole of a strong electrolyte AB in 50 moles of the solvent at 283 K (assuming complete dissociation of solute AB).

A solution is prepared by dissolving 5 g of a non-volatile solute in 200 g of water. It has a vapour pressure of 31·84 mm Hg at 300 K. Calculate the molar mass of the solute. (Vapour pressure of pure water at 300 K = 32 mm Hg)

(a) Differentiate between Ideal solution and Non-ideal solution. (b) 30 g of urea is dissolved in 846 g of water. Calculate the vapour pressure of water for this solution if vapour pressure of pure water at 298 K is 23.8 mm Hg.

Give reason: (a) Measurement of osmotic pressure method is preferred for the determination of molar masses of macromolecules such as proteins and polymers. (b) Aquatic animals are more comfortable in cold water than in warm water. (c) Elevation of boiling point of 1 M KCl solution is nearly double than that of 1 M sugar solution.

When 19.5 g of F–CH2–COOH (Molar mass = 78 g mol–1), is dissolved in 500 g of water, the depression in freezing point is observed to be 1°C. Calculate the degree of dissociation of F–CH2–COOH. [Given: Kf for water = 1.86 K kg mol–1]

0.3 g of acetic acid (M = 60 g mol⁻¹) dissolved in 30 g of benzene shows a depression in freezing point equal to 0.45°C. Calculate the percentage association of acid if it forms a dimer in the solution. (Given: Kf for benzene = 5.12 K kg mol⁻¹)

If benzoic acid (M = 122 g mol^-1) is associated into a dimer when dissolved in benzene and the osmotic pressure of a solution of 6.1 g of benzoic acid in 100 mL benzene is 6.5 atm at 27°C, then what is the percentage association of benzoic acid? (Given: R = 0.0821 L atm K^-1 mol^-1)

Write three differences between Lyophobic sol and Lyophilic sol.

(a) (i) Calculate the freezing point of a solution when 10·5 g of MgBr2 was dissolved in 250 g of water, assuming MgBr2 undergoes complete dissociation. (Given : Molar mass of MgBr2 = 184 g mol⁻¹, Kf for water = 1·86 K kg mol⁻¹) (ii) Write two differences between ideal and non-ideal solutions.

(a) (i) Calculate the freezing point of a solution when 10·5 g of MgBr2 was dissolved in 250 g of water, assuming MgBr2 undergoes complete dissociation. (Given: Molar mass of MgBr2 = 184 g mol⁻¹, Kf for water = 1·86 K kg mol⁻¹) (ii) Write two differences between ideal and non-ideal solutions. OR (b) (i) A solution is prepared by dissolving 0·025 g of potassium sulphate in 2 L of water at 27°C. Assuming potassium sulphate is completely dissociated, determine its osmotic pressure. (Given: R = 0·082 L atm K⁻¹ mol⁻¹, Molar mass of K2SO4 = 174 g mol⁻¹) (ii) What type of azeotrope will be formed by a solution of acetone and chloroform? Give reason.

(A) (a) Calculate the boiling point of solution when 6 g of MgSO4 (Molar mass = 120 g mol–1) was dissolved in 200 g of water, assuming the complete dissociation of MgSO4. (Kb for water = 0.52 K kg mol–1). (b) State Raoult's law for a solution containing volatile components. How Raoult's law is a special case of Henry's law ?

(a) (i) At the same temperature, CO2 gas is more soluble in water than O2 gas. Which one of them will have higher value of KH and why? (ii) How does the size of blood cells change when placed in an aqueous solution containing more than 0·9% (mass/volume) sodium chloride? (iii) 1 molal aqueous solution of an electrolyte A2B3 is 60% ionized. Calculate the boiling point of the solution. (Given : Kb for H2O = 0·52 K kg mol1)

(a) (i) At the same temperature, CO2 gas is more soluble in water than O2 gas. Which one of them will have higher value of KH and why?

(a) (i) Why is boiling point of 1M NaCl solution more than that of 1M glucose solution? (ii) A non-volatile solute 'X' (molar mass = 50 g mol–1) when dissolved in 78g of benzene reduced its vapour pressure to 90%. Calculate the mass of X dissolved in the solution. (iii) Calculate the boiling point elevation for a solution prepared by adding 10g of MgCl2 to 200g of water assuming MgCl2 is completely dissociated.

(a) (i) Why is boiling point of 1M NaCl solution more than that of 1M glucose solution? (ii) A non-volatile solute 'X' (molar mass = 50 g mol–1) when dissolved in 78g of benzene reduced its vapour pressure to 90%. Calculate the mass of X dissolved in the solution. (iii) Calculate the boiling point elevation for a solution prepared by adding 10g of MgCl2 to 200g of water assuming MgCl2 is completely dissociated. (Kb for Water = 0.512 K kg mol–1, Molar mass MgCl2 = 95g mol–1)

The standard electrode potentials of three metals A, B and C are, respectively, + 0·34 V, − 1·18 V and − 0·25 V. The correct order of reducing power of these metals is :

1. B > C > A
2. A > B > C
3. C > B > A
4. A > C > B

What will happen during the electrolysis of aqueous solution of CuCl2 by using platinum electrodes?

1. Cu will deposit at Anode
2. H2 gas will be released at cathode
3. O2 gas will be released at anode
4. Cl2 gas will be released at anode

How many Faradays are required to reduce 1 mol of Cr2O7²⁻ to Cr³⁺ in acidic medium?

1. 2
2. 3
3. 6
4. 4

How the conductivity varies on decreasing concentration for both weak and strong electrolytes ?

1. It increases for weak electrolyte and decreases for strong electrolyte.
2. It decreases for weak electrolyte and increases for strong electrolyte.
3. It increases for both weak and strong electrolytes.
4. It decreases for both weak and strong electrolytes.

Consider the following reaction: Zn (s) + Ag2O(s) + H2O(l) → Zn2+(aq) + 2Ag(s) + 2OH–(aq). Given: EoAg+/Ag = 0.80 V, EoZn2+/Zn = – 0.76 V, 1 F = 96500 C mol–1. ΔrGo for the above reaction is:

1. – 301.080 kJ mol–1
2. + 310.080 kJ mol–1
3. –326.070 kJ mol–1
4. –375.060 kJ mol–1

Consider the following reaction: Zn (s) + Ag2O(s) + H2O(l) → Zn2+(aq) + 2Ag(s) + 2OH–(aq). Given: E°Ag+/Ag = 0.80 V, E°Zn2+/Zn = – 0.76 V, 1 F = 96500 C mol–1. ΔrG° for the above reaction is:

1. – 301.080 kJ mol–1
2. + 310.080 kJ mol–1
3. –326.070 kJ mol–1
4. –375.060 kJ mol–1

On electrolysis of very dilute aqueous solution of NaCl using platinum electrodes:

1. H2 gas is evolved at anode.
2. Na is produced at cathode.
3. O2 gas is evolved at anode.
4. H2 gas is evolved at cathode.

Consider the following cell at 298 K: Mg (s) | Mg2+ (1·0 M) || Cu2+ (1·0 M) | Cu (s). How can we increase the emf of the cell using the same substances?

1. By decreasing only the [Mg2+] to 0·1 M
2. By decreasing only the [Cu2+] to 0·1 M
3. By increasing both [Mg2+] and [Cu2+] to 2·0 M
4. By increasing only the [Mg2+] to 2·0 M

Assertion (A): E°Cu2+/Cu has positive value (+ 0.34 V). Reason (R): It is due to low ∆hydH° and high ∆aH°.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): E°Mn+2/Mn value is highly negative. Reason (R): Because Mn2+ is highly stable due to half-filled 3d5 configuration.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Kohlrausch gave the following relation for strong electrolytes at low concentration: Λm = Λ0m – AC. Which of the following equality holds true ?

1. Λm = Λ0m as C → A
2. Λm = Λ0m as C → 0
3. Λm = Λ0m as C → ∞
4. Λm = Λ0m as C → 1

ΔrG° and Ecell for a spontaneous reaction will respectively be

1. positive and positive
2. positive and negative
3. negative and positive
4. negative and negative

In an electrochemical cell, the following reaction takes place: 2Cu+ (aq) + Zn (s) → 2Cu (s) + Zn2+ (aq), E°cell = 1·28 V. As the reaction progresses, what will happen to the overall voltage of the cell?

1. Voltage will remain constant.
2. It will decrease as [Zn2+] increases.
3. It will increase as [Cu+] increases.
4. It will increase as [Zn2+] increases.

What amount of electric charge is required for the reduction of 1 mole of MnO4– into Mn2+?

1. 1 F
2. 5 F
3. 4 F
4. 6 F

Assertion (A): Electrolysis of aqueous NaCl gives H2 at cathode and Cl2 at anode. Reason (R): Chlorine has higher oxidation potential than H2O.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The product of the oxidation of I– with MnO4– in alkaline medium is:

1. IO4–
2. I2
3. IO–
4. IO3–

In an electrochemical cell, the following reaction takes place: 2Ag+ (aq) + Mg (s) → 2Ag (s) + Mg2+ (aq), Ecell = 2·96 V. As the reaction progresses, what will happen to the overall voltage of the cell?

1. Voltage will remain constant.
2. It will decrease as [Mg2+] increases.
3. It will increase as [Ag+] increases.
4. It will increase as [Mg2+] increases.

What amount of electric charge is required for the oxidation of 1 mole of H2O to O2?

1. 1F
2. 2F
3. 3F
4. 4F

In an electrochemical cell, the following reaction takes place: 2Cu+ (aq) + Zn (s) → 2Cu (s) + Zn2+ (aq) with E°cell = 1·28 V. As the reaction progresses, what will happen to the overall voltage of the cell?

1. Voltage will remain constant.
2. It will decrease as [Zn2+] increases.
3. It will increase as [Cu+] increases.
4. It will increase as [Zn2+] increases.

What amount of electric charge is required for the oxidation of 1 mole of FeO to Fe2O3?

1. 1F
2. 2F
3. 3F
4. 4F

Match the type of cell given in Column I with their use given in Column II. Column I: i. Lead storage cell ii. Mercury cell iii. Dry cell iv. Fuel cell Column II: a. Wall clock b. Apollo Space Programme c. Wrist watch d. Inverter

1. i-a, ii-b, iii-c, iv-d
2. i-d, ii-c, iii-a, iv-b
3. i-c, ii-d, iii-b, iv-a
4. i-b, ii-a, iii-d, iv-c

Assertion (A): For measuring resistance of an ionic solution an AC source is used. Reason (R): Concentration of ionic solution will change if DC source is used.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

While doing qualitative analysis in chemistry lab, Abhishek added yellow coloured potassium chromate solution into a test tube. He was surprised to see the colour of the solution changing immediately to orange. He realised that the test tube was not clean and contained a few drops of some liquid. Which of the following substances will be the most likely liquid to be present in the test tube before adding potassium chromate solution?

1. Sodium hydrogen carbonate solution
2. Methyl orange solution
3. Sodium hydroxide solution
4. HCl solution

Which of the following cell converts the energy of combustion of fuel into electrical energy ?

1. Mercury cell
2. Fuel cell
3. Dry cell
4. Lead storage cell

A galvanic cell can behave like an electrolytic cell when

1. Ecell = Eext
2. Eext > Ecell
3. Ecell > Eext
4. Ecell = 0

We cannot measure the resistance of an ionic solution using DC because:

1. it changes the composition of the solution.
2. it can cause sparks and shocks.
3. it does not affect the composition of the solution.
4. it converts electrolytic cell to galvanic cell.

During electrolysis of dilute H2SO4, using platinum electrodes, the gas evolved at the anode is :

1. H2 gas
2. O2 gas
3. SO2 gas
4. SO3 gas

Kohlrausch gave the following relation for strong electrolytes: Λm = Λ°m – A√C. Which of the following equality holds true ?

1. Λm = Λ°m as C → 1
2. Λm = Λ°m as C → 0
3. Λm = Λ°m as C → ∞
4. Λm = Λ°m as C → A

A conductivity cell usually consists of two:

1. Copper electrodes
2. Platinum electrodes
3. Zinc electrodes
4. Iron electrodes

The equilibrium Cr2O7²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H2O exists in:

1. basic medium
2. acidic medium
3. neutral medium
4. does not exist

During electrolysis of aqueous solution of NaCl:

1. H2 (g) is liberated at cathode
2. Na is formed at cathode
3. O2 (g) is liberated at anode
4. Cl2 (g) is liberated at cathode

The product of oxidation of SO3^2- with MnO4^- in acidic medium is:

1. SO2
2. SO4^2-
3. S2
4. S2O3^2-

During electrolysis of aqueous CuCl2:

1. H2 (g) is liberated at cathode
2. Cu is formed at cathode
3. O2 (g) is liberated at anode
4. Cl2 (g) is liberated at cathode

The unit of cell constant is:

1. ohm cm⁻¹
2. ohm⁻¹
3. cm⁻¹
4. ohm⁻¹ cm² mol⁻¹

During the electrolysis of aqueous NaCl, the cathodic reaction is :

1. Oxidation of Cl ion
2. Reduction of Na+ ion
3. Oxidation of H2O
4. Reduction of H2O

Which of the following is a secondary cell?

1. Dry cell
2. Lead storage cell
3. Mercury cell
4. Daniell cell

Which of the following cells is used in hearing aids?

1. Dry cell
2. Mercury cell
3. Nickel-cadmium cell
4. Fuel cell

The correct cell to represent the following reaction is: Zn + 2Ag+ → Zn2+ + 2Ag

1. 2Ag | Ag+ || Zn || Zn2+
2. Ag+ | Ag || Zn2+ | Zn
3. Ag | Ag+ || Zn | Zn2+
4. Zn | Zn2+ || Ag+ | Ag

ΔG and Ecell for a spontaneous reaction will be:

1. positive, negative
2. negative, negative
3. negative, positive
4. positive, positive

Ag+ (aq) + e⁻ → Ag (s) E° = + 0.80 V Fe²⁺ (aq) + 2e⁻ → Fe (s) E° = −0.44 V Find the cell E° for: Fe (s) + 2Ag+ (aq) → Fe²+ (aq) + 2Ag (s)

1. 1.6 V
2. 1.16 V
3. 2.04 V
4. 1.24 V

Which of the following solutions of KCl will have the highest value of molar conductivity?

1. 0.01 M
2. 1 M
3. 0.5 M
4. 0.1 M

Assertion (A): Conductivity decreases with decrease in concentration of electrolyte. Reason (R): Number of ions per unit volume that carry the current in a solution decreases on dilution.

1. Both (A) and (R) are true and (R) is the correct explanation of (A)
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A)
3. (A) is true, but (R) is false
4. (A) is false, but (R) is true

Which of the following relations is incorrect?

1. R = 1/(k × l/a)
2. G = k × a/l
3. G = k × l/a
4. m = k/c

Assertion (A): Molar conductivity decreases with increase in concentration. Reason (R): When concentration approaches zero, the molar conductivity is known as limiting molar conductivity.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3. (A) is true, but (R) is false.
4. (A) is false, but (R) is true.

Assertion (A): Electrolysis of aqueous solution of NaCl gives chlorine gas at anode instead of oxygen gas. Reason (R): Formation of oxygen gas at anode requires overpotential.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Kohlrausch gave the following relation for strong electrolyte: Λ = Λ₀ - A√C. Which of the following equality holds true?

1. Λ₀ = Λ as C → A
2. Λ₀ = Λ as C → 0
3. Λ₀ = Λ as C → ∞
4. Λ₀ = Λ as C → 1

KMnO4 acts as an oxidising agent in alkaline medium. When alkaline KMnO4 is treated with KI, iodide ion is oxidised to:

1. I2
2. IO⁻
3. IO₃⁻
4. IO₄⁻

The cathode reaction during the charging of a lead storage battery leads to the:

1. formation of PbSO₄
2. reduction of Pb²⁺ to Pb⁴⁺
3. formation of PbO₂ and Pb
4. deposition of Pb at the anode

How many Faradays are required to reduce 1 mol of MnO4^- to Mn2+?

1. 4
2. 3
3. 6
4. 5

Assertion (A): λm for weak electrolytes shows a sharp decrease when the electrolytic solution is diluted. Reason (R): For weak electrolytes, degree of dissociation increases with dilution of solution.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The number of faradays passed through a solution of CuSO₄ to produce 1 mol of Cu and O₂ will be:

1. 10
2. 40
3. 80
4. 20

Assertion (A): Λm for weak electrolytes shows a sharp increase when the electrolytic solution is diluted. Reason (R): For weak electrolytes, degree of dissociation decreases with dilution of solution.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Corrosion of iron is:

1. a decomposition process
2. a photochemical process
3. an electrochemical process
4. a reduction process

Assertion (A): Limiting molar conductivity (Λₘ) is obtained by the extrapolation of the Λₘ versus C^(1/2) curve of strong electrolyte. Reason (R): Λₘ for weak electrolytes is obtained by using Kohlrausch law.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): Cu/2Cu⁺ E° is positive (+0.34 V). Reason (R): Copper has high Δ_hyd H and low Δ_hydr H.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

A voltaic cell is made by connecting two half cells represented by half equations below: Sn2+(aq) + 2e– → Sn(s) E = –0.14 V; Fe3+(aq) + e– → Fe2+(aq) E = +0.77 V. Which statement is correct about this voltaic cell?

1. Fe2+ is oxidised and the voltage of the cell is –0.91 V
2. Sn is oxidised and the voltage of the cell is 0.91 V
3. Fe2+ is oxidised and the voltage of the cell is 0.91 V
4. Sn is oxidised and the voltage of the cell is 0.63 V

Which of the following cell was used in Apollo space programme?

1. Mercury cell
2. Daniel cell
3. H2–O2 Fuel cell
4. Dry cell

Consider the following standard electrode potential values: Fe3+(aq) + e– → Fe2+(aq) E = + 0.77 V and MnO4–(aq) + 8H+ + 5e– → Mn2+(aq) + 4 H2O(l) E = + 1.51 V. What is the cell potential for the redox reaction?

1. – 2.28 V
2. – 0.74 V
3. + 0.74 V
4. + 2.28 V

A voltaic cell is made by connecting two half cells represented by half equations below: Sn2+(aq) + 2e– → Sn(s) E = – 0.14 V and Fe3+(aq) + e– → Fe2+(aq) E = + 0.77 V. Which statement is correct about this voltaic cell?

1. Fe2+ is oxidised and the voltage of the cell is –0.91 V
2. Sn is oxidised and the voltage of the cell is 0.91 V
3. Fe2+ is oxidised and the voltage of the cell is 0.91 V
4. Sn is oxidised and the voltage of the cell is 0.63 V

Consider the following standard electrode potential values: Sn2+(aq) + 2e– → Sn(s) E = – 0.14 V and Fe3+(aq) + e– → Fe2+(aq) E = + 0.77 V. What is the cell reaction and potential for the spontaneous reaction that occurs?

1. 2 Fe2+(aq) + Sn2+(aq) → 2 Fe3+(aq) + Sn(s) E = – 0.91 V
2. 2 Fe3+(aq) + Sn(s) → 2 Fe2+(aq) + Sn2+(aq) E = + 0.91 V
3. 2 Fe2+(aq) + Sn2+(aq) → 2 Fe3+(aq) + Sn(s) E = + 0.91 V
4. 2 Fe3+(aq) + Sn(s) → 2 Fe2+(aq) + Sn2+(aq) E = + 1.68 V

(a) Name the cell which was used in the Apollo space programme for providing electrical power. (b) Define limiting molar conductivity.

(a) Name any two materials other than hydrogen that can be used as fuel in fuel cells. (b) Define molar conductivity.

(a) Name the cell used in hearing aids and watches. (b) Define conductivity. Why is direct current (DC) not used for the measurement of resistance of an ionic solution?

(a) Why does the cell potential of mercury cell remains constant throughout its life ? (b) Calculate the degree of dissociation (α) of CH3COOH if Λm and Λ0m of CH3COOH are 50 S cm2 mol–1 and 400 S cm2 mol–1 respectively.

Using the E° values of P and Q, predict which one is better for coating the surface of iron [E°(Fe2+ → Fe) = –0.44 V] to prevent corrosion and why ? E°(P2+ → P) = –2.37 V, E°(Q2+ → Q) = –0.14 V

Define fuel cell. Give two advantages of fuel cell over ordinary cell.

Name and define the cell which was used for providing electric power in the Apollo space programme. Also write its one advantage.

Based on the data given: Concentration of KCl solution in mol/L (1.000, 0.100, 0.010), Conductivity at 298.15 K in S cm–1 (0.1113, 0.0129, 0.00141), Molar Conductivity at 298.15 K in S cm2 mol–1 (111.3, 129.0, 141.0). Give plausible reason for the variation of conductivity and molar conductivity with concentration.

Calculate the potential of Iron electrode in which the concentration of Fe2+ ion is 0.01 M. (EoFe2+/Fe = -0.45 V at 298 K) [Given: log 10 = 1]

Calculate the potential of Iron electrode in which the concentration of Fe2+ ion is 0.01 M. (E°Fe2+/Fe = -0.45 V at 298 K) [Given: log 10 = 1]

What is meant by conductivity? Give an application.

On diluting two electrolytes A and B 5 times, the molar conductivity of A becomes 25 while that of B is 1.5. Which of the two electrolytes is strong? Justify your answer graphically.

Complete the following equations: (a) 4MnO2 + 2NO5 + 6H+ → (b) Cr2O7 + 14H+ + 6e- →

(a) The E° value for the Mn³⁺/Mn²⁺ couple is much more positive than that for Cr³⁺/Cr²⁺ couple or Fe³⁺/Fe²⁺ couple. How would you account for this? (b) Complete the following equation: 4MnO₂ + 16H⁺ + 24e⁻ → 2O₂C₅...

(a) On diluting two electrolytes A and B their λₘ values are 5 S cm² mol⁻¹ and 1.5 S cm² mol⁻¹ respectively. Which of the two electrolytes is strong? Justify your answer graphically. OR (b) The electrical resistance of a column of 0.05 mol L⁻¹ NaOH solution of diameter 1 cm and length 50 cm is 5.55 × 10⁻³ ohm. Calculate the conductivity.

(a) Calculate ΔrG for the cell reaction at 25°C: Zn | Zn2+ || Cd2+ | Cd. Given that: E°Zn/2Zn = −0.76 V, E°Cd/2Cd = −0.40 V, 1 F = 96500 C mol−1. OR (b) The electrical resistance of a column of 0.05 mol L−1 NaOH solution of diameter 1 cm and length 50 cm is 5.55 × 10−3 ohm. Calculate the conductivity.

Complete the following equations: (a) 4MnO2 + 2NO3− + 6H+ → (b) Cr2O7²⁻ + 14H+ + 6e− →

Give reasons: (i) Mercury cell delivers a constant potential during its life time. (ii) In the experimental determination of electrolytic conductance, Direct Current (DC) is not used.

(a) Give reasons: (i) Mercury cell delivers a constant potential during its life time. (ii) In the experimental determination of electrolytic conductance, Direct Current (DC) is not used. OR (b) Define fuel cell with an example. What advantages do the fuel cells have over primary and secondary batteries?

Define fuel cell and write its two advantages.

Name the cell which: (a) was used in Apollo Space programme. (b) is used in automobiles and inverters. (c) is suitable for hearing aids and watches. (d) does not give a steady potential and is used in transistors.

(a) (i) What should be the signs (positive/negative) for ECell and ΔG for a spontaneous redox reaction occurring under standard conditions? (ii) State Faraday's first law of electrolysis.

(a)(i) What should be the signs (positive/negative) for ECell and G for a spontaneous redox reaction occurring under standard conditions?

Define molar conductivity for the solution of an electrolyte. How does it vary with concentration ?

The resistance and conductivity of a conductivity cell containing 0·001 M KCl solution at 298 K are 1200 Ω and 1·5 × 10⁻⁴ S cm⁻¹. Calculate its cell constant and molar conductivity.

In a plot of m against the square root of concentration (C1/2) for strong and weak electrolyte, the value of limiting molar conductivity of a weak electrolyte cannot be obtained graphically. Suggest a way to obtain this value. Also state the related law, if any.

Define conductivity and molar conductivity for a solution of an electrolyte. Why does the conductivity of a solution decrease with decrease in concentration ?

Answer the following: (i) Why is the Equilibrium Constant (Kc) related to E°cell and not to Ecell? (ii) Two metals 'A' and 'B' have standard electrode potential values of –0.24 V and +0.80 V respectively. Which of these will liberate hydrogen gas from dil. H2SO4? (iii) Write the cell reaction which occurs in lead storage battery when it is in charging.

Calculate emf of the following cell at 298 K: Sn | Sn2+(0.001 M) || H+(0.01 M) | H2(g) (1 bar) | Pt(s). Given: EoSn2+/Sn = – 0.14 V, EoH+/H2 = 0.00 V [log 10 = 1]

Calculate emf of the following cell at 298 K: Sn | Sn 2+ (0.001 M) | | H+ (0.01 M) | H2(g) (1 bar) | Pt(s). Given: E°Sn2+/Sn = – 0.14 V, E°H+/H2 = 0.00 V [log 10 = 1]

State Kohlrausch's law of independent migration of ions. With the help of a curve, explain why it is not easy to determine λ_m for weak electrolytes by extrapolating the concentration − molar conductivity curve, as it is for strong electrolytes.

Answer the following questions: (a) Why is direct current (DC) not used to measure the resistance of an ionic solution? (b) Why are the products of electrolysis different for the electrolysis of aqueous solution of AgNO3 with silver electrodes and electrolysis of aqueous solution of AgNO3 with platinum electrodes? (c) Why are magnesium blocks fixed to the iron pipelines carrying water?

(a) Why is direct current (DC) not used to measure the resistance of an ionic solution? (b) Why are the products of electrolysis different for the electrolysis of aqueous solution of AgNO3 with silver electrodes and electrolysis of aqueous solution of AgNO3 with platinum electrodes? (c) Why are magnesium blocks fixed to the iron pipelines carrying water?

Calculate emf of the following cell at 298 K : Cr (s)| Cr³⁺(aq) (0.1 M)|| Fe²⁺(aq) (0.01 M)|Fe (s) (Given : E°Cr³⁺/Cr = – 0.74 V, E°Fe²⁺/Fe = – 0.44 V, [log 10 = 1])

Calculate emf of the following cell at 298 K: Al (s)| Al³⁺(aq) (0.1 M)|| Ni²⁺(aq) (0.01 M)|Ni (s). (Given: E°(Ni²⁺/Ni) = –0.25 V, E°(Al³⁺/Al) = –1.66 V, [log 10 = 1])

Calculate emf of the following cell at 298 K: Zn (s)|Zn²⁺ (aq) (0.1 M)|| Ag⁺ (aq) (0.01 M)|Ag (s) (Given: E°(Zn²⁺/Zn) = –0.76 V, E°(Ag⁺/Ag) = +0.80 V, [log 10 = 1])

Calculate ΔrG° and log KC for the following cell at 25°C : Zn | Zn2+ || Cd2+ | Cd Given that : E°(Zn2+ → Zn) = –0.76 V, E°(Cd2+ → Cd) = –0.40 V 1 F = 96500 C mol–1.

Calculate the cell voltage of the voltaic cell which is set up by joining following half-cells at 25°C: Al/ Al3+ (0.001 M) and Ni/ Ni2+ (0.1 M). Given: E°(Ni2+/Ni) = –0.25 V, E°(Al3+/Al) = –1.66 V

Calculate the cell voltage of the voltaic cell which is set up by joining the following half-cells at 25°C: Al/ Al3+ (0·001 M) and Ni/ Ni2+ (0·001 M). Given: Eo(Ni2+/Ni) = – 0·25 V, Eo(Al3+/Al) = – 1·66 V

Calculate the cell voltage of the voltaic cell which is set up by joining the following half-cells at 25°C: Al/Al³⁺ (0·002 M) and Ni/Ni²⁺ (0·002 M). Given: E°Ni²⁺/Ni = –0·25 V, E°Al³⁺/Al = –1·66 V, log 5 = 0·6990

Give reasons for the following: (a) The pH of aqueous NaCl increases when it is electrolysed. (b) Unlike dry cell, mercury cell has a constant cell potential through its lifetime. (c) Conductivity of solution decreases with dilution.

Write the name of the cell which is generally used in inverters. Write the reactions taking place at anode and cathode of this cell, when it is in use.

(a) Write the name of the cell which is generally used in inverters. Write the reactions taking place at anode and cathode of this cell, when it is in use. OR (b) Explain why electrolysis of an aqueous solution of NaCl gives H2 gas at cathode and Cl2 gas at anode? Write overall reaction. (Given: E°Na+/Na = – 2.71 V, E°H2O/H2 = – 0.83 V, E°Cl2/2Cl– = + 1.36 V, E°O2/H2O = + 1.23 V)

When a certain conductivity cell was filled with 0.05 M KCl solution, it has a resistance of 100 ohm at 25°C. When the same cell was filled with 0.02 M AgNO3 solution, the resistance was 90 ohm. Calculate the conductivity and molar conductivity of AgNO3 solution. (Given: Conductivity of 0.05 M KCl solution = 1.35×10-2 ohm-1cm-1)

When a certain conductivity cell was filled with 0.05 M KCl solution, it has a resistance of 100 ohm at 25ºC. When the same cell was filled with 0.02 M AgNO3 solution, the resistance was 90 ohm. Calculate the conductivity and molar conductivity of AgNO3 solution. (Given: Conductivity of 0.05 M KCl solution = 1.35×10⁻² ohm⁻¹cm⁻¹)

Calculate emf of the following cell: Zn (s) | Zn2+ (0.1 M) || Sn2+ (0.001 M) | Sn (s) [log 10 = 1]

The conductivity of 0·2 M solution of KCl is 2·48 × 10⁻² S cm⁻¹. Calculate its molar conductivity and degree of dissociation (α). Given: λ°ₖ = 73·5 S cm² mol⁻¹, λ°ₓₗ = 76·5 S cm² mol⁻¹

The conductivity of 0·2 M solution of KCl is 2·48 × 10-2 S cm-1. Calculate its molar conductivity and degree of dissociation (α). Given: λoK = 73·5 S cm2 mol-1, λoCl = 76·5 S cm2 mol-1

The conductivity of 0.2 M solution of KCl is 2.48 × 10⁻² S cm⁻¹. Calculate its molar conductivity and degree of dissociation (α). Given: λ°ₖ = 73.5 S cm² mol⁻¹ and λ°ᶜˡ = 76.5 S cm² mol⁻¹

Calculate the degree of dissociation (α) of CH3COOH if Λm and Λ₀m of CH3COOH are 48 S cm² mol⁻¹ and 400 S cm² mol⁻¹ respectively.

Calculate the emf of the following cell: Zn (s)|Zn²⁺ (0·01 M) || (0·001 M) Ag⁺|Ag (s) Given: E°Zn/Zn² = −0·76 V and E°Ag/Ag = +0·80 V [log 2 = 0·3010, log 3 = 0·4771, log 10 = 1]

Calculate the emf of the following cell : Zn (s)|Zn²⁺ (0·01 M) || Ag⁺ (0·001 M) Ag (s) Given : E°(Zn/Zn²⁺) = -0·76 V and E°(Ag/Ag⁺) = +0·80 V [log 2 = 0·3010, log 3 = 0·4771, log 10 = 1]

Write the Nernst equation and calculate emf of the following cell at 298 K: Cr|Cr3+ (0·1 M)||Fe2+ (0·01 M)|Fe Given: Cr3+/Cr E° = -0.75 V; Fe2+/Fe E° = -0.45 V (log 10 = 1)

Write the Nernst equation and calculate the emf of the following cell at 298 K: Zn|Zn2+ (0·001 M)| |H+ (0·01 M)|H2 (g) (1 bar)|Pt (s) Given: Zn2+/Zn E° = -0·76 V, 2H+/H2 E° = 0·00 V [log 10 = 1]

Write the Nernst equation and calculate the emf of the following cell at 298 K: Zn|Zn2+ (0.1 M)| |Cd2+ (0.01)|Cd Given: E°Zn2+/Zn = -0.76 V, E°Cd2+/Cd = -0.40 V (log 10 = 1)

Write the Nernst equation and calculate the emf of the following cell at 298 K : Mg (s)Mg2+ (0·001 M) || Cu2+ (0·0001 M)Cu (s) Given : E°Mg2+/Mg = − 2·36 V, E°Cu2+/Cu = + 0·34 V [log 10 = 1]

From the given data of E values, answer the following questions: E°(M2+/M) V: Cr –1.18, Mn –0.91, Fe –1.18, Co –0.44, Ni –0.28, Cu –0.25, Cu +0.34. (I) Why E°(M2+/M) show irregular trend in the above values? (II) Why is E°(Cu2+/Cu) value exceptionally positive? (III) Why E°(Mn2+/Mn) value is highly negative?

Calculate emf and ΔG for the following cell at 298 K: Mg(s) / Mg2+(0.01 M) // Ag+(0.001 M) / Ag(s). Given: E°(Mg2+/Mg) = –2.37 V, E°(Ag+/Ag) = +0.80 V. [1 F = 96500 C mol–1, log 10 = 1]

Calculate emf and ΔG for the following cell at 298 K: Mg(s) / Mg²⁺(0.01 M) // Ag⁺(0.001 M) / Ag(s). Given: E°(Mg²⁺/Mg) = –2.37 V, E°(Ag⁺/Ag) = +0.80 V [Note: 1 F = 96500 C mol⁻¹, log 10 = 1]

The conductivity of 0.1 mol L–1 solution of NaCl is 1.06 × 10–2 S cm–1. Calculate its molar conductivity and degree of dissociation. (Given: λo(Na+) = 50.1 S cm2 mol–1, λo(Cl–) = 76.5 S cm2 mol–1). Following cell reaction occurs in a galvanic cell: 2Ag+(aq) + Zn(s) → 2Ag(s) + Zn2+(aq) E°(cell) = +1.56 V. Predict the direction of flow of current. Differentiate between a primary battery and a secondary battery.

(a) The conductivity of 0.1 mol L–1 solution of NaCl is 1.06 × 10–2 S cm–1. Calculate its molar conductivity and degree of dissociation. °Na+ = 50.1 S cm2 mol–1, °Cl– = 76.5 S cm2 mol–1 (b) (i) Following cell reaction occurs in a galvanic cell : 2Ag +(aq) + Zn(s) — 2Ag(s) + Zn2+(aq) E°(cell) = +1.56 V. Predict the direction of flow of current. (ii) Differentiate between a primary battery and a secondary battery.

(a) The conductivity of 0.1 mol L–1 solution of NaCl is 1.06 × 10–2 S cm–1. Calculate its molar conductivity and degree of dissociation. (Given: Λ°Na+ = 50.1 S cm2 mol–1, Λ°Cl– = 76.5 S cm2 mol–1) (b) (i) Following cell reaction occurs in a galvanic cell: 2Ag +(aq) + Zn(s) — 2Ag(s) + Zn2+(aq) E°(cell) = +1.56 V. Predict the direction of flow of current. (ii) Differentiate between a primary battery and a secondary battery.

Calculate the electrode potential of a half-cell for zinc electrode dipping in 0·01 M ZnSO4 solution at 25°C. Given: E°(Zn2+/Zn) = − 0·76 V [log 10 = 1]. Write anode, cathode and overall reaction involved in dry cell. Equilibrium constant (Kc) is related to E°cell, but not to Ecell. Why?

(a) (i) Calculate the electrode potential of a half-cell for zinc electrode dipping in 0·01 M ZnSO4 solution at 25°C. Given: E°(Zn2+/Zn) = − 0·76 V [log 10 = 1]

(a) Calculate the electrode potential of a half-cell for zinc electrode dipping in 0·01 M ZnSO4 solution at 25°C. Given: E°(Zn2+/Zn) = − 0·76 V [log 10 = 1] (ii) Write anode, cathode and overall reaction involved in dry cell. (iii) Equilibrium constant (Kc) is related to E°cell, but not to Ecell. Why ?

(a)(i) Calculate Eocell for the following reaction which is at equilibrium: Cu (s) + 2Ag+(aq) ⇌ Cu2+(aq) + 2Ag (s). Equilibrium constant (Kc) for the cell is 1015. [Given: log 10 = 1] (ii) Write anode, cathode and overall reaction of lead storage battery when it is in use. (iii) How much electricity is required in coulombs for the oxidation of 1 mol of FeO to Fe2O3?

(a)(i) Calculate E°cell for the following reaction which is at equilibrium: Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s). Equilibrium constant (Kc) for the cell is 1015. [Given: log 10 = 1] (ii) Write anode, cathode and overall reaction of lead storage battery when it is in use. (iii) How much electricity is required in coulombs for the oxidation of 1 mol of FeO to Fe2O3?

(a)(i) For a galvanic cell, the following half reactions are given. Decide, which will remain as reduction reaction and which will be reversed to become an oxidation reaction. Give reason for your answer. (I) Cr3+ + 3e– → Cr(s); E = – 0·74 V (II) Fe2+ + 2e– → Fe(s); E = – 0·44 V

For a galvanic cell, the following half reactions are given. Decide, which will remain as reduction reaction and which will be reversed to become an oxidation reaction. Give reason for your answer. (I) Cr3+ + 3e– → Cr(s); E = –0·74 V (II) Fe2+ + 2e– → Fe(s); E = –0·44 V. Represent the cell in which the following reaction takes place: Mg(s) + 2Ag+ (0·001 M) → Mg2+ (0·100 M) + 2Ag(s). Calculate Ecell if E°cell = 3·17 V. (log 10 = 1)

(a) (i) Calculate Ecell of a galvanic cell in which the following reaction takes place at 25°C: Zn(s) + Pb2+(0·02 M) → Zn2+(0·1 M) + Pb(s) [Given: E°Zn2+/Zn = – 0·76 V, E°Pb2+/Pb = – 0·13 V; log 2 = 0·3010, log 4 = 0·6021, log 5 = 0·6990]. (ii) State Faraday's first law of electrolysis. How much electricity, in terms of Faraday, is required to reduce one mol of MnO4– to Mn2+ ion ?

(a) (i) Calculate Ecell of a galvanic cell in which the following reaction takes place at 25C: Zn(s) + Pb2+(0·02 M) → Zn2+(0·1 M) + Pb(s) [Given: EZn/Zn2+ = – 0·76 V, EPb/Pb2+ = – 0·13 V; log 2 = 0·3010, log 4 = 0·6021, log 5 = 0·6990] OR (b) (i) The resistance of a conductivity cell containing 0·001 M KCl solution at 298 K is 1000 ohm. What is the cell constant if conductivity of 0·001 M KCl solution at 298 K is 0·125 × 10–3 S cm–1?

Calculate E°cell of a galvanic cell in which the following reaction takes place at 25C: Zn(s) + Pb²⁺(0·02 M) → Zn²⁺(0·1 M) + Pb(s) [Given: E°Zn²⁺/Zn = – 0·76 V, E°Pb²⁺/Pb = – 0·13 V; log 2 = 0·3010, log 4 = 0·6021, log 5 = 0·6990]

Calculate the emf of the following cell at 25°C: Zn(s)|Zn2+ (0.1 M) || H+ (0.01 M)|H2(g) (1 bar), Pt(s). (Given : E°(Zn2+/Zn) = – 0.76 V, E°(H+/H2) = 0.00 V, log 10 = 1). State Faraday's second law of electrolysis. How much electricity is required in terms of Faraday for the reduction of 1 mol of Cr2O72– to Cr3+ ?

Calculate the emf of the following cell at 25°C: Zn(s)|Zn2+ (0.1 M) || H+ (0.01 M)|H2(g) (1 bar), Pt(s) [Given: E°Zn2+/Zn = –0.76 V, E°H2+/H2 = 0.00 V, log 10 = 1]

(a) (i) Calculate the emf of the following cell at 25°C: Zn(s)|Zn2+ (0.1 M) || H+ (0.01 M)|H2(g) (1 bar), Pt(s) [Given: E°Zn2+/Zn = – 0.76 V, E°H+/2H2 = 0.00 V, log 10 = 1] (ii) State Faraday's second law of electrolysis. How much electricity is required in terms of Faraday for the reduction of 1 mol of Cr2O72– to Cr3+?

(a) (i) The resistance of 0.05 M CH3COOH solution is found to be 100 ohm. If the cell constant is 0.0354 cm^-1, calculate the molar conductivity of the acetic acid solution. (ii) How much charge in Faraday is required for the reduction of 1 mol of MnO4^- to Mn^2+?

(a) The resistance of 0.05 M CH₃COOH solution is found to be 100 ohm. If the cell constant is 0.0354 cm⁻¹, calculate the molar conductivity of the acetic acid solution. (b) State Faraday's law. How many Faradays are required for the reduction of 1 mol of MnO₄⁻ to Mn²⁺?

(a) (i) Calculate emf of the following cell at 25ºC : Zn (s) Zn²⁺ (0·001M) ∥ Cd²⁺ (0·1 M) Cd (s) Given : E°Zn²⁺/Zn = -0·76 V, E°Cd²⁺/Cd = -0·40 V [log 10 = 1]

Calculate emf of the following cell at 25ºC: Zn (s) | Zn2+ (0·001M) || Cd2+ (0·1 M) | Cd (s). Given: EoZn2+/Zn = -0·76 V, EoCd2+/Cd = -0·40 V [log 10 = 1] OR State Faraday's second law of electrolysis. How will the pH of aqueous NaCl solution be affected when it is electrolysed?

Calculate emf of the following cell at 25°C: Zn (s) | Zn²⁺ (0.001M) || Cd²⁺ (0.1 M) | Cd (s). Given: E°(Zn²⁺/Zn) = −0.76 V, E°(Cd²⁺/Cd) = −0.40 V [log 10 = 1]

(a) (i) Write an expression for the limiting molar conductivity of an acetic acid on the basis of Kohlrausch law. (ii) Calculate the maximum work and log Kc for the given reaction at 298 K: Ni (s) + 2Ag+ (aq) → Ni2+ (aq) + 2Ag (s). Given: Ni/Ni2+ E° = -0.25 V, Ag+/Ag E° = +0.80 V, 1 F = 96500 C mol-1

(a) (i) Write an expression for the molar conductivity of acetic acid at infinite dilution according to Kohlrausch law. (ii) Calculate the maximum work and log Kc for the given reaction at 298 K: Ni (s) + 2Ag⁺ (aq) → Ni²⁺ (aq) + 2Ag (s). Given: E°(Ni/Ni²⁺) = −0.25 V, E°(Ag/Ag⁺) = +0.80 V, 1 F = 96500 C mol⁻¹ OR (b) (i) Write Faraday's first law of electrolysis. How many Faradays of electric charge are required for the reduction of 1 mol Cu²⁺ to Cu? (ii) Calculate emf of the following cell at 298 K: Mg (s) | Mg²⁺ (0.1 M) || Cu²⁺ (0.1 M) | Cu (s). [E°cell = +2.71 V, 1 F = 96500 C mol⁻¹, log 10 = 1]

(a) (i) Write an expression for the limiting molar conductivity of acetic acid. (ii) Calculate the maximum work and log Kc for the given reaction at 298 K: Ni (s) + 2Ag+ (aq) → Ni2+ (aq) + 2Ag (s). Given: E°Ni/2Ni = −0.25 V, E°Ag/Ag = +0.80 V, 1 F = 96500 C mol−1. OR (b) (i) How many Faraday of electricity, in terms of Faraday, is required for the reduction of 1 mol Cu2+ to Cu? (ii) Calculate emf of the following cell at 298 K for Mg (s) | Mg2+ (0.1 M) || Cu2+ (0.1 M) | Cu (s). [E°cell = +2.71 V, 1 F = 96500 C mol−1, log 10 = 1]

Conductivity of 2×10–3 M methanoic acid is 8×10–5 S cm–1. Calculate its molar conductivity and degree of dissociation if λ°m for methanoic acid is 404 S cm2 mol–1.

Conductivity of 2 × 10–3 M methanoic acid is 8 × 10–5 S cm–1. Calculate its molar conductivity and degree of dissociation if λ°m for methanoic acid is 404 S cm2mol–1. Calculate the ΔrG and log Kc for the given reaction at 298 K: Ni (s) + 2Ag+(aq) → Ni2+(aq) + 2Ag(s). Given: E Ni2+/Ni = – 0.25 V, E°Ag+/Ag = +0.80 V, 1F = 96500 C mol –1.

(a) Conductivity of 2 × 10–3 M methanoic acid is 8 × 10–5 S cm–1. Calculate its molar conductivity and degree of dissociation if Λ⁰m for methanoic acid is 404 S cm2mol–1. (b) Calculate the ΔrG and log Kc for the given reaction at 298 K: Ni (s) + 2Ag+(aq) → Ni2+(aq) + 2Ag(s) Given: E°Ni2+/Ni = – 0.25 V, E°Ag+/Ag = +0.80 V; 1F = 96500 C mol–1.

(a) Calculate the emf of the following cell at 25°C: Zn(s) | Zn²⁺(0.1 M) || H⁺(0.01 M) | H2(g)(1 bar), Pt(s) [Given: E°(Zn²⁺/Zn) = -0.76 V, E°(2H⁺/H2) = 0.00 V, log 10 = 1]

(a) Calculate the emf of the following cell at 25°C: Zn (s) | Zn²⁺ (0.1 M) || H⁺ (0.01 M) | H2 (g) (1 bar), Pt (s). (Given: E°Zn/2Zn = −0.76 V, E°2H/H = 0.00 V, log 10 = 1) (b) State Kohlrausch law of independent migration of ions. Why does the conductivity of a solution decrease with dilution?

Calculate the emf of the following cell at 25°C: Zn (s) | Zn²⁺ (0.1 M) || H⁺ (0.01 M) | H₂ (g) (1 bar), Pt (s)

(a) (i) Calculate the emf of the following cell at 298 K: Al (s) | Al3+ (0.001 M) || Ni2+ (0.1 M) | Ni (s). [Given: E°(Al/3Al) = -1.66 V, E°(Ni/2Ni) = -0.25 V, log 10 = 1]

(a) (i) Calculate the emf of the following cell at 298 K: Al (s) | Al³⁺ (0.001 M) || Ni²⁺ (0.1 M) | Ni (s). [Given: E°(Al/³⁺Al) = -1.66 V, E°(Ni/²⁺Ni) = -0.25 V, log 10 = 1] (ii) With the help of a graph explain why it is not possible to determine Λ°m for a weak electrolyte by extrapolating the molar conductivity (Λm) versus C^(1/2) curve as for strong electrolyte.

The rate of a reaction is doubled when the concentration of the reactant is doubled. The order of the reaction is :

1. 0
2. 1
3. 2
4. 0·5

Assertion (A) : Rate of reaction increases with an increase in temperature. Reason (R) : Number of effective collisions decreases with an increase in temperature.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following curve represents the first order reaction?

1. A
2. B
3. C
4. D

For a reaction: N2 + 3H2 → 2NH3, the rate of reaction with respect to NH3 is

1. +1/3 d[NH3]/dt
2. -1/2 d[NH3]/dt
3. +1/4 d[NH3]/dt
4. +1/2 d[NH3]/dt

Identify the correct statement:

1. Molecularity of a reaction is an experimental quantity.
2. For complex reactions molecularity has no meaning.
3. Molecularity of a reaction can be zero or even a fraction.
4. Molecularity more than three is very common in chemical reactions.

The order for the given reaction is: A + 2B → Products, Rate = k[A]½[B]1

1. 1.5
2. 1
3. 0.5
4. 2

Assertion (A): The molecularity of the given reaction is 2. 2HI → H2 + I2. Reason (R): Two molecules of the reactants are involved in simultaneous collision between them.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

For a reaction 3A → 2B, the rate of reaction +d[B]/dt is equal to:

1. -3/2 d[A]/dt
2. -2/3 d[A]/dt
3. -1/3 d[A]/dt
4. +d[A]/2 dt

Assertion (A): Order of reaction is applicable to elementary as well as complex reactions. Reason (R): Order of a reaction is an experimental quantity.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

For the reaction 2A → 3B, the rate of reaction +d[B]/dt is equal to :

1. 3/2 × (-d[A]/dt)
2. 2/3 × (-d[A]/dt)
3. 1/2 × (-d[A]/dt)
4. 3 × (d[A]/dt)

Assertion (A): Order of reaction is not applicable for elementary reaction but applicable for complex reaction. Reason (R): Order of reaction is an experimental quantity.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The half-life periods of decomposition of NH3 for different initial pressures are given below: p (torr) 704, 75, 34·5; t1/2 (min) 80, 80, 80. The order of the reaction is :

1. zero order
2. first order
3. 0·5
4. second order

The rate of a first order reaction is 5·6 × 10–4 mol L–1 s–1, when the concentration of reactant is 0·2 mol L–1. The rate constant 'k' is:

1. 5·6 × 10–3 s–1
2. 2·8 × 10–4 s–1
3. 2·8 × 10–5 s–1
4. 2·8 × 10–3 s–1

Assertion (A): For complex reaction, order of reaction is given by the slowest step. Reason (R): Order of a reaction is an experimental quantity.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): For complex reaction, order of reaction is given by the fast step. Reason (R): Order of reaction is determined experimentally.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): For complex reaction, order of reaction is given by the slowest step. Reason (R): Order of reaction is not applicable for the complex reaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Half-life (t1/2) of a first order reaction is 1386 s. The value of rate constant is :

1. 0·5 × 10⁴ s⁻¹
2. 5·0 × 10⁻⁴ s⁻¹
3. 0·5 × 10⁻⁵ s⁻¹
4. 0·5 × 10⁻² s⁻¹

The rate of reaction X + Y → products, is given by the equation Rate = k[X] [Y]. If Y is taken in large excess, the order of the reaction would be

1. 0
2. 1
3. 2
4. 1/2

Assertion (A): In a first order reaction, if the concentration of the reactant is doubled, its half-life is also doubled. Reason (R): The half-life of a reaction does not depend upon the initial concentration of the reactant in a first order reaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

The role of a catalyst is to change:

1. equilibrium constant
2. enthalpy of reaction
3. Gibbs energy of reaction
4. activation energy of reaction

The unit of rate and rate constant are same for a :

1. First order reaction
2. Second order reaction
3. Zero order reaction
4. Third order reaction

Assertion (A) : Hydrolysis of an ester follows first order kinetics. Reason (R) : The concentration of water does not get altered much during the reaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The value of rate constant for a pseudo first order reaction:

1. depends only on temperature.
2. depends on the concentration of reactants present in small amount.
3. depends on the concentration of reactants present in large excess.
4. is not dependent on the concentration of reactants.

Assertion (A): Order of the reaction can be zero or fractional. Reason (R): We cannot determine order from balanced chemical equation.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

In the Arrhenius equation k = Ae^(–Ea/RT), 'A' represents:

1. effective collisions
2. frequency factor
3. fraction of collisions
4. threshold energy

Assertion (A): Molecularity of reaction is determined experimentally. Reason (R): Molecularity is applicable only for an elementary reaction and not for a complex reaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The activation energy (Ea) of a reaction can be determined from the slope of which of the following plots ?

1. ln k vs. T
2. ln(k/T) vs. T
3. ln k vs. 1/T
4. ln(T/k) vs. 1/T

Unit of rate constant 'k' for a second order reaction is :

1. s–1
2. mol L–1 s–1
3. mol–1 L s–1
4. mol–2 L s–1

Which of the following represents the fraction of molecules with energies equal to or greater than Ea ?

1. e^(-Ea/RT)
2. e^(T-Ea/RT)
3. e^(T+Ea/RT)
4. e^(Ea+E/RT)

Which of the following is the slope of the first order reaction in the plot of ln[R] vs. time?

1. + k
2. + k/2.303
3. – k
4. – k/2.303

In the Arrhenius equation, when log k is plotted against 1/T, a straight line is obtained whose:

1. slope is AR and intercept is Ea.
2. slope is A and intercept is aER.
3. slope is aERTand intercept is log A.
4. slope is R303·2aE and intercept is log A.

A reaction A2 + B2 → 2AB occurs by the following mechanism: A2 → A + A (slow); A + B2 → AB + B (fast); A + B → AB (fast). Its order would be:

1. 1
2. 2
3. Zero
4. 1/2

A zero-order reaction is one whose rate is independent of:

1. Presence of light
2. Concentration of the reactant
3. Temperature of the reaction
4. Pressure of the reaction

The addition of catalyst during a chemical reaction alters which of the following quantities of the reaction?

1. Enthalpy
2. Activation energy
3. Entropy
4. Internal energy

For the elementary reaction P→Q, when the concentration of P is doubled, the rate of reaction becomes 8 times. The order of the reaction is:

1. 3
2. 4
3. 2
4. 1

Half-life period of a first order reaction is 1386 seconds. The rate constant (k) of the reaction is:

1. 0.5 × 10^-3 s^-1
2. 5.0 × 10^-3 s^-1
3. 5 × 10^-2 s^-1
4. 0.5 × 10^-2 s^-1

The rate of the reaction 2A + B2 → 2AB is given by Rate = k [A]^2 [B2]. The value of rate constant (k) can be increased by:

1. increasing the concentration of A
2. increasing the concentration of B
3. increasing the temperature
4. all the above three

For a certain reaction R → products, a plot of log [R] vs. time gives a straight line with a slope of −1.25 s⁻¹. The order of the reaction is:

1. One
2. Zero
3. Two
4. Fractional

For a zero order reaction A → products, t₁/₂ is:

1. [A]₀/k
2. 0.693/k
3. [A]₀/2k
4. [A]₀²/2k

When a catalyst increases the rate of a chemical reaction, then the rate constant (k) :

1. remains constant
2. decreases
3. increases
4. may increase or decrease depending on the order of the reaction

Assertion (A): Order of reaction and molecularity are always same for complex reactions. Reason (R): Order is determined experimentally and molecularity is applicable only for elementary reactions.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

When the initial concentration of a reactant is doubled in the reaction, the half life period remains same. The order of reaction is:

1. First
2. Second
3. Zero
4. 1/2

Assertion (A): Rate of reaction increases with increase in temperature. Reason (R): Number of effective collisions increase with increase in temperature.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The half-life of a first-order reaction with rate constant (k) of 3 min⁻¹ is:

1. 0.693 min
2. 2.31 min
3. 6.93 min
4. 0.231 min

Assertion (A): Rate of reaction decreases with increase in temperature. Reason (R): Number of effective collisions increases with increase in temperature.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Which of the following is affected by catalyst?

1. ΔH
2. ΔG
3. Ea
4. ΔS

The order of the reaction H2 (g) + Cl2 (g) → 2HCl (g) is:

1. 2
2. 1
3. 0
4. 3

Assertion (A): The molecularity of the reaction H2 + Br2 → 2HBr appears to be 2. Reason (R): Two molecules of the reactants are involved in the given elementary reaction. Select the correct answer.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

A first order reaction takes 30 minutes for 50% completion. The value of rate constant k would be:

1. 2.5 × 10⁻³ min⁻¹
2. 2.75 × 10⁻⁴ min⁻¹
3. 1.25 × 10⁻³ min⁻¹
4. 2.31 × 10⁻³ min⁻¹

Assertion (A): The molecularity of the reaction H₂ + Br₂ → 2HBr appears to be 2. Reason (R): Two molecules of the reactants are involved in the given elementary reaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The slope in the plot of ln[R] vs. time for a first order reaction is

1. +k/2.303
2. –k
3. –k/2.303
4. +k

For the reaction 3A → 2B, rate of reaction +d[B]/dt is equal to

1. –3/2 d[A]/dt
2. –2/3 d[A]/dt
3. –1/3 d[A]/dt
4. +2 d[A]/dt

The slope in the plot of [R] vs. time for a zero order reaction is

1. + k/2.303
2. – k
3. – k/2.303
4. + k

For a reaction 2A → 3B, rate of reaction – d[A]/dt is equal to

1. + 3/2 d[B]/dt
2. + 2/3 d[B]/dt
3. + 1/3 d[B]/dt
4. + 2 d[B]/dt

The slope in the plot of log R/R₀ vs. time for a first order reaction is

1. + k/2.303
2. + k
3. – k/2.303
4. – k

For the reaction 3A → 2B, rate of reaction – d[A]/dt is equal to

1. +(3/2) × d[B]/dt
2. +(2/3) × d[B]/dt
3. +(1/3) × d[B]/dt
4. +(1/2) × d[B]/dt

The unit of the rate of reaction is the same as that of the rate constant for a:

1. first order reaction
2. second order reaction
3. zero order reaction
4. it cannot be same

Assertion (A): Order and molecularity of a reaction are always same. Reason (R): Complex reactions involve a sequence of elementary reactions and the slowest step is rate determining.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The rate of reaction A + B → Products, is given by the equation r = k[A] [B]. If B is taken in large excess, the order of reaction would be:

1. 2
2. 0
3. 1
4. Cannot be predicted

The half-life of a reaction is doubled when the initial concentration is doubled. The order of the reaction is:

1. 1
2. 2
3. 4
4. 0

The half-life for a zero order reaction equals:

1. R/k2
2. 2R/k2^1
3. k2/R2
4. k2/R

In a reaction, the initial concentration of the reactants increases four fold and the rate becomes sixteen times its initial value. The order of the reaction is:

1. 2.0
2. 3.5
3. 1.5
4. 2.5

For the reaction A + 2B → C + D, the rate law is given by r = k[A][B]², the concentration of A is kept constant while that of B is doubled. The rate of the reaction will:

1. double
2. become half
3. not change
4. quadruple

If the initial concentration is reduced to 1/4th in a zero order reaction, then the time taken for half the reaction to complete:

1. remains the same
2. reduces to one-fourth
3. increases four times
4. doubles

For a zero order reaction of the type A → products, the rate equation may be expressed as:

1. t = [A]/k₀
2. t = [A]₀/k
3. t = [A]₀/2k
4. t = [A]₀²/2k

The number of molecules that react with each other in an elementary reaction is a measure of the:

1. activation energy of the reaction
2. order of the reaction
3. stoichiometry of the reaction
4. molecularity of the reaction

The following experimental rate data were obtained for a reaction carried out at 25 C: A (g) + B(g) → C(g) + D(g). What are the orders with respect to A(g) and B(g)?

1. Zero; Second
2. First; Zero
3. Second; Zero
4. Second; First

Assertion (A): For a zero order reaction the unit of rate constant and rate of reaction are same. Reason (R): Rate of reaction for zero order reaction is independent of concentration of reactant.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): The half life of a reaction is the time in which the concentration of the reactant is reduced to one half of its initial concentration. Reason (R): In first order kinetics when concentration of reactant is doubled, its half life is doubled.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): Order of reaction is applicable to elementary as well as complex reactions. Reason (R): For a complex reaction molecularity has no meaning.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Write any two differences between the order of a reaction and molecularity of a reaction.

Following reaction takes place in one step: 2A + B → 2C. How will the rate of above reaction change if the volume of the reaction vessel is decreased to one third of its original volume? Will there be any change in the order of reaction with the reduced volume?

The concentration of the reactant is reduced from 0.6 mol L–1 to 0.2 mol L–1 in 5 minutes in a first order reaction. Calculate rate constant of the reaction. (log 3 = 0.48)

Define activation energy. Write the unit of rate constant for (i) zero order reaction, (ii) second order reaction.

(a) Define Collision frequency. (b) Write the units of (i) first order reaction and (ii) zero order reaction

(a) Define Effective collision. (b) Write the unit of (i) second order reaction and (ii) zero order reaction

For a reaction A + B → Products, the rate law is: Rate = k[A][B]^(3/2). Write the overall order of the reaction. Can this reaction be an elementary reaction? Give reason in support of your answer.

For a reaction A + B → Products, the rate law is: Rate = (3/2)k[A][B]^2. Write the overall order of the reaction. Can this reaction be an elementary reaction ? Give reason in support of your answer.

For a reaction A + B → Products, the rate law is: Rate = (3/2)k[A][B]. Write the overall order of the reaction. Can this reaction be an elementary reaction ? Give reason in support of your answer.

(a) Reactions of which order will show the rate to be independent of the concentration of the reactant? Give one example of this order. (b) State the condition under which a bimolecular reaction may be kinetically a first order reaction.

(a) A reaction is second order in 'A' and first order in 'B'. How is the rate affected when the concentrations of both 'A' and 'B' are doubled ? (b) Write the unit of 'k' for zero order reaction.

(a) The reaction between A2 (g) and B2 (g) was carried out in a sealed isothermal container. The rate law for the reaction was found to be: Rate = k[A2][B2]. If 1 mole of A2 (g) was added to the reaction chamber and the temperature was kept constant, then predict the change in rate of the reaction and the rate constant.

(a) Write the rate law expression for the reaction 2HI → H2 + I2, if the order of the reaction is zero.

Define rate constant and identify the reaction order which has a rate constant of 4·5 × 10–5 L mol–1 s–1.

Give any two differences between order and molecularity of a reaction.

State a condition under which a bimolecular reaction is kinetically first order reaction. Give an example. For which type of reactions, do order and molecularity have the same value ?

Why is molecularity applicable only for elementary reactions and order is applicable for elementary as well as complex reactions?

Define molecularity of the reaction. State any one condition in which a bimolecular reaction may be kinetically of first order.

Write two differences between order of reaction and molecularity of reaction.

A first order reaction has a rate constant 1.25×10−3 s−1. How long will 5 g of this reactant take to reduce to 2.5 g? [log 2 = 0·301, log 3 = 0·4771, log 4 = 0·6021]

(a) In a reaction, when the concentration of a reactant is tripled, the rate of the reaction becomes twenty-seven times. What is the order of the reaction ?

When the initial concentration of a reactant is tripled, the reaction rate becomes twenty-seven times. What is the order of the reaction? OR State a condition under which a bimolecular reaction is kinetically a first-order reaction. Give an example of such a reaction.

If the concentration of a reactant in a reaction becomes twenty-seven times, the rate of reaction becomes twenty-seven times. What is the order of the reaction?

The conversion of molecule A to B followed second order kinetics. If concentration of A increased to three times, how will it affect the rate of formation of B?

(a) The conversion of molecule A to B followed second order kinetics. If concentration of A increased to three times, how will it affect the rate of formation of B? (b) Define Pseudo first order reaction with an example.

A chemical reaction 2N2O5(g) → 4NO2(g) + O2(g) in gas phase was carried out in a closed vessel. The concentration of NO2 was found to increase by 5×10⁻³ mol L⁻¹ in 10 seconds. Calculate: (a) the rate of formation of NO2, and (b) the rate of consumption of N2O5.

The following data were obtained for the reaction: 2NO2 (g) + F2 (g) → 2NO2F (g). Experiment No. 1: [NO2]/M = 0.2, [F2]/M = 0.05, Initial rate M min⁻¹ = 6×10⁻³. Experiment No. 2: [NO2]/M = 0.4, [F2]/M = 0.05, Initial rate M min⁻¹ = 12×10⁻². Experiment No. 3: [NO2]/M = 0.8, [F2]/M = 0.10, Initial rate M min⁻¹ = 48×10⁻². Determine the overall order of reaction.

The half-life of a first order reaction is 60 minutes. How long will it take to consume 90% of the reactant?

The rate constant for the first order decomposition of N2O5 is given by the following equation: log k = 236 - (TK/1024). Calculate Ea for this reaction. [R = 8.314 J K^-1 mol^-1]

The rate constant for the first order decomposition of N₂O₅ is given by the following equation: log k = 23.6 - 1024/T(K). Calculate Ea for this reaction. [R = 8.314 J K⁻¹ mol⁻¹]

What happens to the rate constant k and activation energy Ea as the temperature of a chemical reaction is increased? Justify.

In a reaction 2N2O5 (g) → 4NO2 (g) + O2 (g), the concentration of N2O5 decreases from 0·5 mol L⁻¹ to 0·4 mol L⁻¹ in 10 minutes. Calculate the average rate of this reaction and rate of production of NO2 during this period.

A reaction is first order in X and second order in Y. (i) How is the rate affected on increasing the concentration of Y three times? (ii) How is the rate affected when the concentrations of both X and Y are doubled?

A first order reaction is 50% complete in 20 minutes. Calculate the time for 75% completion of the reaction. [log 4 = 0·6]

For the first order thermal decomposition reaction, following data was obtained: C2H5Cl(g) → C2H4(g) + HCl(g). S. No. Time(s) Total Pressure (atm) 1 0 0.30 2 30 0.50. Calculate rate constant. [Given: log 3 = 0.48]

The half-life period of a radioactive element is 1·5 × 10^10 years. Calculate the time in which the activity of the element is reduced to 75% of its original value. [Given: log 2 = 0·30, log 3 = 0·48, log 4 = 0·60]

Consider the decomposition of hydrogen peroxide (H2O2) as per the equation given below: 2H2O2 → 2H2O + O2 (I– catalyst). The mechanism for this reaction was found to be: Step I: H2O2 + I– → H2O + IO– (slow). Step II: H2O2 + IO– → H2O + I– + O2 (fast). (a) Write the rate law expression. (b) Determine the order of reaction with respect to H2O2, I– and overall order of reaction. (c) What is the molecularity of the reaction in Step II?

Consider the decomposition of hydrogen peroxide (H2O2) as per the equation given below: 2H2O2 —[I,Alkaline medium]→ 2H2O + O2. The mechanism for this reaction was found to be: Step I: H2O2 + I– → H2O + IO– (slow), Step II: H2O2 + IO– → H2O + I– + O2 (fast). (a) Write the rate law expression. (b) Determine the order of reaction with respect to H2O2, I– and overall order of reaction. (c) What is the molecularity of the reaction in Step II?

(a) Define order of a reaction. (b) The rate for the following reaction is given by : A + B → C, Rate = k[A][B]². (i) How is the rate of reaction affected if we double the concentration of B ? (ii) Write the overall order of a reaction if 'A' is present in large excess.

The rate of the chemical reaction doubles when the temperature is raised from 298 K to 308 K. Calculate activation energy (Ea) for this reaction assuming that it does not change with temperature. (Given : R = 8·314 J mol⁻¹ K⁻¹, log 2 = 0·30)

The rate of a particular reaction quadruples when the temperature increases from 293 K to 313 K. Calculate the energy of activation (Ea) of the reaction assuming that it does not change with temperature. (Given: log 4 = 0·60, R = 8·314 JK⁻¹ mol⁻¹)

The rate of a particular reaction quadruples when the temperature increases from 300 K to 320 K. Calculate the energy of activation (Ea) of the reaction assuming that it does not change with temperature. (Given: log 4 = 0·60, R = 8·314 JK⁻¹ mol⁻¹)

The rate constant of a first order reaction increases from 0.04 s–1 to 0.08 s–1 when the temperature increases from 27°C to 37°C. Calculate the energy of activation (Ea). [Given : 2.303R = 19.15 JK–1mol–1] [log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021]

For the reaction A + B → Products, the following initial rates were obtained at various initial concentrations of reactants: Sl. No. 1: [A]=0.1 mol L–1, [B]=0.1 mol L–1, Initial rate=0.05 mol L–1 s–1; Sl. No. 2: [A]=0.2 mol L–1, [B]=0.1 mol L–1, Initial rate=0.10 mol L–1 s–1; Sl. No. 3: [A]=0.1 mol L–1, [B]=0.2 mol L–1, Initial rate=0.05 mol L–1 s–1. Determine the order of the reaction with respect to A and B and overall order of the reaction.

For the reaction A + B → Products, the following initial rates were obtained at various initial concentrations of reactants: Sl. No. 1: [A]/mol L–1 = 0·1, [B]/mol L–1 = 0·1, Initial rate/mol L–1 s–1 = 0·05; Sl. No. 2: [A]/mol L–1 = 0·2, [B]/mol L–1 = 0·1, Initial rate/mol L–1 s–1 = 0·10; Sl. No. 3: [A]/mol L–1 = 0·1, [B]/mol L–1 = 0·2, Initial rate/mol L–1 s–1 = 0·05. Determine the order of the reaction with respect to A and B and overall order of the reaction.

The rate of a reaction : A + B → product is given below as a function of different initial concentrations of A and B. Calculate the order of the reaction with respect to A and B. Determine the rate constant of the reaction.

The following data were obtained during the first order thermal decomposition of N2O5 (g) at constant volume: 2N2O5 (g) → 2N2O4 (g) + O2 (g). S.No. Time/s Total Pressure/atm: 1) 0 0.5, 2) 100 0.625. Calculate rate constant. (Given : log 2 = 0.3010, log 10 = 1)

The following data were obtained during the first order thermal decomposition of N2O5 (g) at constant volume: 2N2O5 (g) → 2N2O4 (g) + O2 (g). S.No. 1: Time 0 s, Total Pressure 0.5 atm; S.No. 2: Time 100 s, Total Pressure 0.625 atm. Calculate rate constant. [Given: log 2 = 0.3010, log 10 = 1]

The following initial rate data were obtained for the reaction: 2NO(g) + Br2(g) → 2NOBr(g). Expt. No. 1: [NO]=0.05, [Br2]=0.05, Rate=1.0×10-3. Expt. No. 2: [NO]=0.05, [Br2]=0.15, Rate=3.0×10-3. Expt. No. 3: [NO]=0.15, [Br2]=0.05, Rate=9.0×10-3. (a) What is the order with respect to NO and Br2 in the reaction? (b) Calculate the rate constant (k). (c) Determine the rate of reaction when concentration of NO and Br2 are 0.4 M and 0.2 M, respectively.

The following initial rate data were obtained for the reaction: 2NO(g) + Br2(g) → 2NOBr(g). Expt. No. | [NO]/mol L⁻¹ | [Br2]/mol L⁻¹ | Initial Rate (mol L⁻¹ s⁻¹) | 1 | 0.05 | 0.05 | 1.0×10⁻³ | 2 | 0.05 | 0.15 | 3.0×10⁻³ | 3 | 0.15 | 0.05 | 9.0×10⁻³ | (a) What is the order with respect to NO and Br2 in the reaction? (b) Calculate the rate constant (k). (c) Determine the rate of reaction when concentration of NO and Br2 are 0.4 M and 0.2 M, respectively.

The rate of a gaseous reaction triples when temperature is increased from 17ºC to 27ºC. Calculate the energy of activation for this reaction. [Given: 2.303 R = 19.15 JK−1 mol−1, log 3 = 0.48]

The rate of a gaseous reaction triples when temperature is increased from 17°C to 27°C. Calculate the energy of activation for this reaction. [Given: 2.303 R = 19.15 J K⁻¹ mol⁻¹, log 3 = 0.48]

A first-order reaction is 25% complete in 40 minutes. Calculate the value of rate constant. In what time will the reaction be 80% complete ? Given : log 2 = 0·30, log 3 = 0·48, log 4 = 0·60, log 5 = 0·69

A first order reaction is 50% complete in 30 minutes at 300 K and in 10 minutes at 320 K. Calculate activation energy (Ea) for the reaction. [R = 8.314 J K–1 mol–1] [Given: log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021]

The rate of a reaction doubles when temperature changes from 27°C to 37°C. Calculate energy of activation for the reaction. (R = 8.314 J K⁻¹ mol⁻¹) (Given: log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021)

The rate of a reaction doubles when temperature changes from 27°C to 37°C. Calculate energy of activation for the reaction. (R = 8.314 J K⁻¹ mol⁻¹)

The following data were obtained during the first order thermal decomposition of C2H5Cl at a constant volume: C2H5Cl (g) → C2H4 (g) + HCl (g). Experiment 1: Time = 0 s, Total pressure = 0.4 atm. Experiment 2: Time = 100 s, Total pressure = 0.6 atm. Calculate the rate constant. [Given: log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021]

(a) For the reaction 2N2O5(g) → 4NO2(g) + O2(g) at 318 K calculate the rate of reaction if rate of disappearance of N2O5(g) is 1.4 × 10–3 m s–1.

(a) For the reaction 2N2O5(g) → 4NO2(g) + O2(g) at 318 K calculate the rate of reaction if rate of disappearance of N2O5(g) is 1.4 × 10–3 m s–1. (b) For a first order reaction derive the relationship t99% = 2t90%

In the given reaction N2 (g) + 3H2 (g) → 2NH3 (g), the rate of formation of NH3 is 3·6 × 10⁻⁴ mol L⁻¹ s⁻¹. Calculate: (i) rate of reaction, and (ii) rate of disappearance of H2 (g).

A first order reduction takes 30 minutes for 75% decomposition. Calculate t₁/₂. Given: [log 2 = 0·3, log 3 = 0·48, log 4 = 0·6, log 5 = 0·7]

A first order reaction takes 30 minutes for 75% decomposition. Calculate t₁/₂. Given: [log 2 = 0·3, log 3 = 0·48, log 4 = 0·6, log 5 = 0·7]

(a) (i) The initial concentration of N2O5 in the first order reaction: N2O5 (g) → 2NO2 (g) + 1/2 O2 (g) was 1.2 × 10–2 mol L–1. The concentration of N2O5 after 60 minutes was 0.2 × 10–2 mol L–1. Calculate the rate constant of the reaction at 318 K. [log 6 = 0.778]

(a) (i) The initial concentration of N2O5 in the first order reaction: N2O5 (g) → 2NO2 (g) + 1/2 O2 (g) was 1·2 × 10⁻² mol L⁻¹. The concentration of N2O5 after 60 minutes was 0·2 × 10⁻² mol L⁻¹. Calculate the rate constant of the reaction at 318 K. [log 6 = 0·778]. (ii) Account for the following: (I) We cannot determine the order of a reaction by taking into consideration the balanced chemical equation. (II) A bimolecular reaction may become kinetically of first order under a specified condition.

Which of the following is not a transition metal ?

1. Hg
2. Cu
3. Ag
4. Pt

Assertion (A) : Transition metals have high melting points. Reason (R) : Transition metals have incompletely filled d-orbitals.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following is most basic?

1. Mn2O7
2. MnO2
3. MnO
4. Mn2O3

Assertion (A): Actinoids show irregularities in their electronic configurations. Reason (R): In actinoids 5f, 6d and 7s orbitals are of comparable energies.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following transition metals has lowest enthalpy of atomisation ?

1. Cr
2. V
3. Mn
4. Fe

Assertion (A) : Actinoids show irregularities in their electronic configurations. Reason (R) : Due to varying stabilities of f0, f7 and f14 occupancies of the 5f orbitals.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Electronic configuration of chromium is:

1. [Ar] 3d4 4s1
2. [Ar] 3d4 4s2
3. [Ar] 3d5 4s1
4. [Ar] 3d5 4s2

Assertion (A): Zinc, cadmium and mercury are not considered as transition elements. Reason (R): These elements have completely filled orbitals in their ground state as well as in their common oxidation states.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

In aqueous solution, Cr2O7(2-) ion converts to which of the following in alkaline medium?

1. Cr3+
2. CrO4(2-)
3. CrO
4. CrO3

Assertion (A): Separation of Zr and Hf is difficult. Reason (R): Because Zr and Hf lie in the same group of the periodic table.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

In aqueous acidified solution, CrO4^2- ion converts to which of the following ?

1. CrO3
2. Cr3+
3. Cr2O7^2-
4. CrO

Assertion (A): Separation of Zr and Hf is difficult. Reason (R): Zr and Hf have almost identical atomic and ionic radii due to lanthanoid contraction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Manganate ion is paramagnetic due to the presence of:

1. one unpaired electron
2. two unpaired electrons
3. three unpaired electrons
4. fully paired electrons

Assertion (A): Eo(Sc3+/Sc2+) has low value. Reason (R): Because of the stability of Sc3+ ion which has a noble gas configuration.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which property of transition metals enables them to form alloys ?

1. High ionization enthalpy
2. Similar atomic radii
3. Catalytic property
4. Complex formation

Which of the following d-orbitals experience more repulsion in the crystal field splitting of octahedral complex?

1. dxy, dyz, dxz
2. dx2–y2, dz2
3. dxy, dx2–y2
4. dxz, dz2

Actinoids show larger number of oxidation states :

1. because they are radioactive in nature
2. because they have large atomic numbers
3. because they have large atomic masses
4. due to comparable energies of 5f, 6d and 7s orbitals

Assertion (A) : Highest oxidation state of Mn is +7 in first series of transition elements. Reason (R) : Transition metals exhibit variable oxidation states.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following transition metals does not show variable oxidation states ?

1. Cu
2. Sc
3. Ti
4. Fe

Assertion (A): Zinc is not regarded as a transition element. Reason (R): Zinc has completely filled 3d orbitals in its ground state as well as in its oxidised state.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Out of Fe3+, Sc3+, Cr3+ and Co3+ ions, the one which is colourless in aqueous solution is: [Atomic number: Fe = 26, Sc = 21, Cr = 24, Co = 27]

1. Sc3+
2. Fe3+
3. Cr3+
4. Co3+

Out of the following statements, the incorrect statement is:

1. La is actually an element of transition series.
2. Zr and Hf have almost identical atomic radii because of lanthanoid contraction.
3. Ionic radius decreases from La3+ to Lu3+ ion.
4. Lanthanoids are radioactive in nature.

The product of the oxidation of I– with MnO4– in alkaline medium is:

1. IO4–
2. I2
3. IO–
4. IO3–

Assertion (A): Cuprous salts are diamagnetic. Reason (R): Cuprous ion has completely filled 3d-orbitals.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Out of Ti3+, Cr3+, Mn2+ and Ni2+ ions, the one which has the highest magnetic moment is: [Atomic number: Ti = 22, Cr = 24, Mn = 25, Ni = 28]

1. Ti3+
2. Cr3+
3. Mn2+
4. Ni2+

Assertion (A): Cuprous salts are diamagnetic. Reason (R): In cuprous ion, 3d-orbitals are partially filled.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Out of Ti3+, Cr3+, Fe2+ and Ni2+ ions, the one which is the most stable ion in aqueous solution is: [Atomic number: Ti = 22, Cr = 24, Fe = 26, Ni = 28]

1. Ti3+
2. Cr3+
3. Fe2+
4. Ni2+

Out of the following statements, the correct statement is:

1. La is actually not an element of transition series.
2. Zr and Hf have almost identical atomic radii.
3. Lanthanoids are radioactive.
4. Ionic radius increases from La3+ to Lu3+.

Which of the following properties of transition metals enables them to behave as catalysts?

1. High melting point
2. High ionisation enthalpy
3. Alloy formation
4. Variable oxidation states

In which of the following groups are both ions coloured in aqueous solution? I. Cu+ II. Ti4+ III. Co2+ IV. Fe2+ [Atomic number: Cu = 29, Ti = 22, Co = 27, Fe = 26]

1. I and II
2. II and III
3. III and IV
4. I and IV

Which of the following is the softest metal ?

1. Zn
2. Sc
3. Cu
4. Fe

Assertion (A) : Actinoids show wide range of oxidation states. Reason (R) : Actinoids are radioactive in nature.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): Actinoids show wide range of oxidation states. Reason (R): This is due to comparable energies of 5f, 6d and 7s orbitals.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following transition metals has the highest melting point?

1. Sc
2. Cr
3. Mn
4. Zn

Assertion (A): Actinoid contraction is greater from element to element than lanthanoid contraction. Reason (R): Actinoids show wide range of oxidation states.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following transition metal ion is not coloured ?

1. Cu+
2. Ni2+
3. Co2+
4. V3+

Assertion (A): Actinoids show irregularities in their electronic configurations. Reason (R): Actinoids are radioactive in nature.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Among the following outermost electronic configurations of transition metals, which one shows the highest oxidation state ?

1. 3d6 4s2
2. 3d5 4s1
3. 3d5 4s2
4. 3d3 4s2

Assertion (A): Actinoids show irregularities in their electronic configurations. Reason (R): This is due to varying stability of f0, f7 and f14 configurations.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

With increase in atomic number, the melting point of transition metals:

1. first increases and then decreases
2. increases continuously
3. first decreases and then increases
4. remains constant

Assertion (A): First ionisation enthalpy of Cr is lower than that of Zn. Reason (R): Zinc is a non-transition element.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which one of the following first row transition elements is expected to have the highest third ionization enthalpy?

1. Iron (Z = 26)
2. Manganese (Z = 25)
3. Chromium (Z = 24)
4. Vanadium (Z = 23)

Assertion (A): Separation of Zr and Hf is difficult. Reason (R): Zr and Hf have similar radii due to lanthanoid contraction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The most stable oxidation state of Iron is:

1. +2
2. +3
3. +4
4. -2

Assertion (A): Transition metals have high enthalpy of atomization. Reason (R): This is because transition metals have low melting points.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): Separation of Zr and Hf is difficult. Reason (R): Zr and Hf are radioactive.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

When MnO2 is fused with KOH in air, it gives:

1. KMnO4
2. K2MnO4
3. Mn2O7
4. Mn2O3

The correct order for the increasing oxidizing power in 3d series of transition elements is:

1. MnO₄ < Cr₂O₇²⁻ < VO₂⁺
2. Cr₂O₇²⁻ < VO₂⁺ < MnO₄
3. VO₂⁺ < Cr₂O₇²⁻ < MnO₄
4. VO₂⁺ < MnO₄ < Cr₂O₇²⁻

Transition elements form alloys easily because they have:

1. same electronic configuration
2. same enthalpies of atomisation
3. same oxidation states
4. nearly the same atomic size

Which of the following elements of 3d series of transition elements has the lowest aHₒ?

1. Sc
2. Cr
3. Cu
4. Zn

The most common and stable oxidation state of a Lanthanoid is:

1. +2
2. +3
3. +4
4. +6

Lanthanoid contraction is due to increase in:

1. atomic number
2. shielding by 4f electrons
3. effective nuclear charge
4. atomic radius

Which of the following characteristics of transition metals is associated with their catalytic activity?

1. Paramagnetic nature
2. Colour of hydrated ions
3. High enthalpy of atomisation
4. Variable oxidation states

Assertion (A): Copper is a non-transition element. Reason (R): Copper has completely filled d-orbitals in its ground state.

1. Both (A) and (R) are true and (R) is the correct explanation of (A)
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A)
3. (A) is true, but (R) is false
4. (A) is false, but (R) is true

Which one among the following metals of 3d series has the lowest melting point ?

1. Fe
2. Mn
3. Zn
4. Cu

Assertion (A): Transition metals have high enthalpy of atomisation. Reason (R): Greater number of unpaired electrons in transition metals results in weak metallic bonding.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3. (A) is true, but (R) is false.
4. (A) is false, but (R) is true.

Which of the following transition metals shows + 1 and + 2 oxidation states?

1. Mn
2. Zn
3. Sc
4. Cu

Assertion (A): Transition metals show their highest oxidation state with oxygen. Reason (R): The ability of oxygen to form multiple bonds to metals.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3. (A) is true, but (R) is false.
4. (A) is false, but (R) is true.

Among the following outermost configurations of transition metals which one shows the highest oxidation state?

1. 3d³4s²
2. 3d⁵4s¹
3. 3d⁵4s²
4. 3d⁶4s²

Assertion (A): Zinc is not regarded as a transition element. Reason (R): In zinc, 3d orbitals are completely filled in its ground state as well as in its oxidised state.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following transition metals does not show variable oxidation state?

1. Ti
2. Cr
3. Cu
4. Sc

Which of the following ions has the maximum number of unpaired d-electrons?

1. Fe³⁺
2. V³⁺
3. Ti³⁺
4. Sc³⁺

Assertion (A): Fe²⁺ acts as a reducing agent. Reason (R): Fe³⁺ state is stable due to 3d⁵ configuration.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The ions of metals of Group 12 (Zn, Cd and Hg) have completely filled d orbitals and so they:

1. behave like semiconductors
2. are very high melting solids
3. do not behave like transition metals
4. behave like superconductors

Assertion (A): Zr and Hf have almost identical radii. Reason (R): Both Zr and Hf exhibit similar properties.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The interstitial compounds of transition metals are:

1. softer
2. more ductile
3. harder
4. more metallic than the metal itself

Assertion (A): Manganese shows the highest oxidation state of +7 in 3d series. Reason (R): Transition metals show variable oxidation states.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Which of the following Cu²⁺ halide is not known?

1. CuBr₂
2. CuI₂
3. CuCl₂
4. CuF₂

Which property of transition metals enables them to behave as catalysts?

1. High melting point
2. High ionisation enthalpy
3. Alloy formation
4. Variable oxidation states

In the two tetrahedral structures of dichromate ion

1. 4 Cr – O bonds are equivalent in length
2. 6 Cr – O bonds are equivalent in length
3. All Cr – O bonds are equivalent in length
4. All Cr – O bonds are non-equivalent

Which of the following ions has the electronic configuration 3d6?

1. Ni3+
2. Co3+
3. Mn2+
4. Mn3+

First ionization enthalpy of Cr is lower than that of Zn. Why? Mention any one property of the transition elements which makes them good catalysts.

(a) Why is third ionization enthalpy of manganese very high ? (b) Why Zn, Cd and Hg are not regarded as transition elements ?

(a) Why second ionization enthalpies of chromium and copper are exceptionally higher than those of their neighbouring elements? (b) Why transition elements form interstitial compounds?

(a) What is lanthanoid contraction? Actinoid contraction is greater from element to element than lanthanoid contraction. Why?

(a) What is lanthanoid contraction? Actinoid contraction is greater from element to element than lanthanoid contraction. Why? OR (b) Why do transition metals have high enthalpy of atomization? Which element of 3d-series has lowest enthalpy of atomization?

Complete the following ionic equations: (a) 42MnO₄⁻ + 35SO₃²⁻ + 6H⁺ →

Complete and balance the following chemical equations: (a) ⁴₃MnO⁴⁻ + 4H⁺ → (b) ₂₇Cr₂O₇²⁻ + 14H⁺ + 6Fe²⁺ →

Complete and balance the following equations: (i) 2KMnO4 → K2MnO4... (ii) Na2Cr2O7 + 2KCl → ... Why is it difficult to separate lanthanoid elements in pure state?

(a) Complete and balance the following equations : (i) 4FeCr 2O4 + 8Na2CO3 + 7O2 –– (ii) 5Fe 2+ + MnO4– + 8H+ –– (b) Explain why actinoid contraction is greater from element to element than lanthanoid contraction.

(a) Complete and balance the following equations: (i) 2Na 2CrO4 + 2H+ –– (ii) 5S 2– + 2MnO4– + 16H+ –– (b) Why is chemistry of actinoids complicated as compared to lanthanoids?

Give explanation for each of the following observations: (a) With the same d-orbital configuration (d4), Mn3+ ion is an oxidising agent whereas Cr2+ ion is a reducing agent. (b) Actinoid contraction is greater from element to element than that among lanthanoids. (c) Transition metals form large number of interstitial compounds with H, B, C and N.

(a) On the basis of crystal field theory write the electronic configuration for d5 ion with a weak ligand for which 0 < P.

From the given E° values of the first row transition elements (Cr = −0·91, Mn = −1·18, Fe = −0·44, Co = −0·28, Ni = −0·25, Cu = +0·34, Zn = −0·76 V), answer the following questions: (i) Why is E°M/²M⁺ value highly negative as compared to other elements for Mn? (ii) What is the reason for the irregularity in the above E° values? (iii) Why is E°Cu/²Cu⁺ value exceptionally positive?

Account for the following: (i) Transition metals and their compounds show catalytic activities. (ii) Zn, Cd and Hg are non-transition elements. (iii) Zr and Hf are of almost identical atomic radii.

From the given E°(M/2M⁺) values of the first row transition elements (Cr: -0·91, Mn: -1·18, Fe: -0·44, Co: -0·28, Ni: -0·25, Cu: +0·34, Zn: -0·76 V), answer the following questions : (i) Why is Mn/2Mn⁺ E° value highly negative as compared to other elements ? (ii) What is the reason for the irregularity in the above E° values ? (iii) Why is Cu/2Cu⁺ E° value exceptionally positive ?

(i) Which ion amongst the following is colourless and why? Ti4+, Cr3+, V3+ (Atomic number of Ti = 22, Cr = 24, V = 23) (ii) Why is Mn2+ much more resistant than Fe2+ towards oxidation? (iii) Highest oxidation state of a metal is shown in its oxide or fluoride only. Justify the statement.

(a) (i) Silver atom has completely filled d-orbitals in its ground state, it is still considered to be a transition element. Justify the statement. (ii) Why are ΔMH°/M2+ values of Mn and Zn more negative than expected? (iii) Why do transition metals form alloys?

(a) (i) Silver atom has completely filled d-orbitals in its ground state, it is still considered to be a transition element. Justify the statement. (ii) Why are M^(M/E2) values of Mn and Zn more negative than expected? (iii) Why do transition metals form alloys?

(b) (i) Calculate the spin only magnetic moment of the complex [Fe(H2O)6]2+. (Atomic number of Fe = 26) (ii) Which out of the following two complexes is more stable and why? [CoF6]3-, [Co(C2O4)3]3- (iii) Write the IUPAC name of the given complex: [Pt(NH3)2Cl2]

(a) (i) Silver atom has completely filled d-orbitals in its ground state, it is still considered to be a transition element. Justify the statement. (ii) Why are M2+/M E° values of Mn and Zn more negative than expected? (iii) Why do transition metals form alloys?

Define transition elements. Mention any two characteristics of transition elements.

(a) (i) From the given data of E values, answer the following questions: (I) Why E(M²⁺/M) show irregular trend in the above values? (II) Why is E(Cu²⁺/Cu) value exceptionally positive? (III) Why E(Mn²⁺/Mn) value is highly negative? (ii) Write the ionic equations for the oxidising action of potassium permanganate for its reaction with I⁻ in both acidic and alkaline solutions.

(a) (i) From the given data of E values, answer the following questions : (I) Why E M2+/M show irregular trend in the above values ? (II) Why is E Cu2+/Cu value exceptionally positive ? (III) Why E Mn2+ / Mn value is highly negative ?

Describe giving reason which one of the following pairs has the property indicated: (I) Fe or Cu − higher melting point (II) Ti3+ or Sc3+ − coloured in aqueous solution (III) Cr or Zn − higher third ionisation enthalpy. Write the ionic equations for the oxidizing action of MnO4^− in acidic medium with: (I) Fe2+ ion (II) I^− ion

(a) (i) Describe giving reason which one of the following pairs has the property indicated: (I) Fe or Cu − higher melting point (II) Ti3+ or Sc3+ − coloured in aqueous solution (III) Cr or Zn − higher third ionisation enthalpy

(a) Describe giving reason which one of the following pairs has the property indicated: (I) Fe or Cu − higher melting point (II) Ti3+ or Sc3+ − coloured in aqueous solution (III) Cr or Zn − higher third ionisation enthalpy (ii) Write the ionic equations for the oxidizing action of MnO4− in acidic medium with: (I) Fe2+ ion (II) I− ion

(a)(i) Account for the following: (I) MnO is basic while Mn2O7 is acidic. (II) Iron has higher enthalpy of atomization than that of copper. (III) Mn3+ is a stronger oxidising agent than Cr3+. (ii) How do you prepare potassium dichromate from sodium chromate? Write balanced chemical equation for each step.

(a) (i) (I) Why do transition metals show variable oxidation states ? (II) Out of Mn²⁺ and Ti²⁺ which will be more paramagnetic and why ? [Atomic No. : Ti = 22, Mn = 25] (III) Which ion is the strongest oxidising agent in the options given below : Cr³⁺, V³⁺, Mn³⁺. Give reason. [Atomic No. : Cr = 24, V = 23, Mn = 25] (ii) Complete and balance the following equations: (I) 2MnO2 + 4KOH + O2 → (II) 5C2O4²⁻ + 2MnO4⁻ + 16H⁺ →

(a) (i) (I) Why do transition metals show variable oxidation states? (I) Out of Mn²⁺ and Ti²⁺ which will be more paramagnetic and why? [Atomic No.: Ti = 22, Mn = 25] (III) Which ion is the strongest oxidising agent in the options given below: Cr³⁺, V³⁺, Mn³⁺. Give reason. [Atomic No.: Cr = 24, V = 23, Mn = 25] (ii) Complete and balance the following equations: (I) 2MnO₂ + 4KOH + O₂ → ? (II) 5C₂O₄²⁻ + 2MnO₄⁻ + 16H⁺ → ?

(A) (a) Account for the following : (i) Transition metals and their compounds show catalytic activities. (ii) Mn3+ is a strong oxidising agent. (iii) Cu+ is not stable in aqueous solution. (b) Write the preparation of KMnO4 from Pyrolusite ore (MnO2).

(a)(i) When pyrolusite ore is fused with KOH, in presence of air, a dark green coloured product 'A' is obtained which changes to purple coloured compound 'B' in acidic medium. (I) Write the formulae of 'A' and 'B'. (II) Write the ionic equation for the reaction when compound 'B' reacts with Fe2+ in acidic medium.

When pyrolusite ore is fused with KOH, in presence of air, a dark green coloured product 'A' is obtained which changes to purple coloured compound 'B' in acidic medium. (I) Write the formulae of 'A' and 'B'. (II) Write the ionic equation for the reaction when compound 'B' reacts with Fe2+ in acidic medium. Give reasons: (I) Ce4+ in aqueous solution is a good oxidising agent. (II) The actinoid contraction is greater from element to element than lanthanoid contraction. (III) E°(Zn2+/Zn) value is more negative than expected, whereas E°(Cu2+/Cu) is positive.

When pyrolusite ore is fused with KOH, in presence of air, a dark green coloured product 'A' is obtained which changes to purple coloured compound 'B' in acidic medium. Write the formulae of 'A' and 'B'.

(a) (i) Account for the following: (I) Orange colour of Cr2O72– ion changes to yellow when treated with an alkali. (II) Zn, Cd and Hg are non-transition elements. (III) E° value for Mn3+/Mn2+ couple is highly positive (+1·57 V) as compared to Cr3+/Cr2+. (ii) What happens when: (I) Manganate ion undergoes disproportionation reaction in acidic medium ? (II) KMnO4 is heated ?

(a) (i) Account for the following: (I) Orange colour of Cr2O72– ion changes to yellow when treated with an alkali. (II) Zn, Cd and Hg are non-transition elements. (III) Eº value for Mn3+/Mn2+ couple is highly positive (+1·57 V) as compared to Cr3+/Cr2+.

Account for the following: (I) Orange colour of Cr2O7²⁻ ion changes to yellow when treated with an alkali. (II) Zn, Cd and Hg are non-transition elements. (III) E° value for Mn³⁺/Mn²⁺ couple is highly positive (+1·57 V) as compared to Cr³⁺/Cr²⁺.

Account for the following: (I) The E°(Mn2+/Mn) value for manganese is highly negative, whereas E°(Mn3+/Mn2+) is highly positive. (II) Actinoids show wide range of oxidation states. (III) Transition metals have high melting points. Complete the following ionic equations: (I) 5SO32– + 2MnO4– + 6H+ → (II) 2MnO4– + H2O + I– →

Account for the following: (I) The E°Mn2+/Mn value for manganese is highly negative, whereas E°Mn3+/Mn2+ is highly positive.

(a) (i) Account for the following: (I) The E°Mn2+/Mn value for manganese is highly negative, whereas E°Mn3+/Mn2+ is highly positive. (II) Actinoids show wide range of oxidation states. (III) Transition metals have high melting points. (ii) Complete the following ionic equations: (I) 5SO32– + 2MnO4– + 6H+ → (II) 2MnO4– + H2O + I– →

(a)(i) Account for the following: (1) The melting and boiling points of Zn, Cd and Hg are low. (2) Of the d4 species, Cr2+ is strongly reducing while Mn3+ is strongly oxidizing. (3) E° value of Cu2+/Cu is +0.34 V. (ii) Complete and balance the following chemical equations: (1) KMnO4 (heat) → (2) Cr2O7(2-) + 6I(-) + 14H+ →

(a) (i) Account for the following: (1) The melting and boiling points of Zn, Cd and Hg are low. (2) Of the d⁴ species, Cr2+ is strongly reducing while Mn3+ is strongly oxidizing. (3) E° value of Cu2+/Cu is +0.34 V.

Assign reason for each of the following: (i) Manganese exhibits the highest oxidation state of +7 among the 3d series of transition elements. (ii) Transition metals and their compounds are generally found to be good catalysts in chemical reactions. (iii) Cr2+ is reducing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidising agent. (iv) Zn has lowest enthalpy of atomization. (v) Cu+ is unstable in an aqueous solution.

(a) (i) In 3d series, which transition element has positive M2+/ME value and why? (ii) Name a member of lanthanide series which is well-known to show +4 oxidation state. (b) Give reason: (i) The highest oxidation state is exhibited in oxoanions of transition metals. (ii) HCl is not used to acidify KMnO4 solution.

Account for the following: (i) Eo value for Mn3+/Mn2+ couple is much more positive than that for Cr3+/Cr2+. (ii) Sc3+ is colourless whereas Ti3+ is coloured in an aqueous solution. (iii) Actinoids show wide range of oxidation states. (iv) Write the chemical equations for the preparation of KMnO4 from MnO2.

Account for the following: (i) E°o value for Mn3+/ Mn2+ couple is much more positive than that for Cr3+/ Cr2+. (ii) Sc3+ is colourless whereas Ti3+ is coloured in an aqueous solution. (iii) Actinoids show wide range of oxidation states. Write the chemical equations for the preparation of KMnO4 from MnO2.

(I) Account for the following: (i) E° value for Mn3+/Mn2+ couple is much more positive than that for Cr3+/Cr2+. (ii) Sc3+ is colourless whereas Ti3+ is coloured in an aqueous solution. (iii) Actinoids show wide range of oxidation states. (II) Write the chemical equations for the preparation of KMnO4 from MnO2. OR (I) Account for the following: (i) Transition metals form alloys. (ii) Ce4+ is a strong oxidising agent. (II) Write one similarity and one difference between chemistry of Lanthanoids and Actinoids. (III) Complete the following ionic equation: Cr2O72– + 2OH– → ___________

(a) (i) Account for the following: (1) Transition metals form complex compounds. (2) The Mn²⁺/Mn value for manganese is highly negative whereas Mn³⁺/Mn²⁺ is highly positive. (3) Cu⁺ ion is unstable in aqueous solution. (ii) Write the equations involved in the preparation of KMnO4 from Pyrolusite ore (MnO2).

(a) (i) Account for the following: (1) Transition metals form complex compounds. (2) The M²⁺/2M E value for manganese is highly negative whereas 2Mn³⁺/3Mn E is highly positive. (3) Cu⁺ ion is unstable in aqueous solution. (ii) Write the equations involved in the preparation of KMnO4 from Pyrolusite ore (MnO2).

Give reasons: (1) Transition metals form complex compounds. (2) The Mn²⁺/Mn³⁺E° value for manganese is highly negative whereas Mn³⁺/MnE° is highly positive. (3) Cu⁺ ion is unstable in aqueous solution.

(a) (i) Account for the following: (1) Zn2+ salts are colourless while Ni2+ salts are coloured. (2) Cr2+ is a strong reducing agent. (3) Transition metals and their compounds show catalytic activities.

(a) (i) Account for the following: (1) Zn²⁺ salts are colourless while Ni²⁺ salts are coloured. (2) Cr²⁺ is a strong reducing agent. (3) Transition metals and their compounds show catalytic activities. (ii) Write the ionic equations for the oxidizing action of MnO₄⁻ in acidic medium with (1) I⁻ ion, and (2) Fe²⁺ ion.

(a) (i) Account for the following: (1) Zn²⁺ salts are colourless while Ni²⁺ salts are coloured. (2) Cr²⁺ is a strong reducing agent. (3) Transition metals and their compounds show catalytic activities. (ii) Write the ionic equations for the oxidizing action of 4MnO₄⁻ in acidic medium with (1) I⁻ ion, and (2) Fe²⁺ ion.

(a) A transition element X has electronic configuration [Ar] 4s2 3d3. Predict its likely oxidation states. (b) Complete the reaction mentioning all the products formed: 2 KMnO4 + heat → (c) Account for the following: (i) In the 3d transition series, zinc has the lowest enthalpy of atomisation, (ii) Cu+ ion is unstable in aqueous solution, (iii) Actinoids show more number of oxidation states than lanthanoids.

(a) Write the number of unpaired electrons in Cr3+. (Atomic number of Cr = 24) (b) Complete the reaction mentioning all the products formed: Cr2O72– + 3H2S + 8H+ → (c) Account for the following: (i) Mn2+ is more stable than Fe2+ towards oxidation to +3 state. (ii) Copper has exceptionally positive EM2+/M value. (iii) Eu2+ with electronic configuration [Xe] 4f76s2 is a strong reducing agent.

The secondary valency of Co in [Co(en)3]2 (SO4)3 is :

1. 12
2. 2
3. 3
4. 6

The secondary valency of Co in the complex [Co(NH3)5(NO2)]2+ is

1. 5
2. 1
3. 4
4. 6

The secondary valency of Pt in [Pt(en)2Cl2]²⁺ is

1. 6
2. 5
3. 4
4. 2

The correct IUPAC name of the complex [Pt(NH3)2Cl2] is:

1. diamminedichloridoplatinum (IV)
2. diamminedichloridoplatinum (II)
3. dichloridodiammineplatinum (IV)
4. dichloridodiammineplatinum (II)

Which of the following is heteroleptic complex?

1. [Co(NH3)6]3+
2. [Cr(NH3)6]3+
3. [Ni(H2O)6]2+
4. [Co(NH3)4Cl2]+

The oxidation number of Co in [Co(en)3]2(SO4)3 is:

1. +3
2. +2
3. +4
4. +6

According to Werner's theory, the primary valencies of the central metal atom:

1. are satisfied by neutral molecules or negative ions.
2. are equal to its coordination number.
3. are satisfied by negative ions.
4. are non-ionisable.

The oxidation number of Co in [Co(NH3)5 (ONO)] SO4 is :

1. + 3
2. + 2
3. + 4
4. + 6

The oxidation number of Pt in [Pt(en)2Cl2]2+ is :

1. + 3
2. + 4
3. + 2
4. + 6

Which of the following d-orbitals experience more repulsion in the crystal field splitting of octahedral complex?

1. dxy, dyz, dxz
2. dx2–y2, dz2
3. dxy, dx2–y2
4. dxz, dz2

The chelating ligand used for the treatment of lead poisoning is:

1. Ethane-1,2-diamine
2. Oxalate ion
3. Dimethylglyoxime
4. EDTA

Which of the following d-orbitals experience more repulsion in the crystal field splitting of tetrahedral complex ?

1. dx2 − y2, dz2
2. dx2 − y2, dxy
3. dxy, dyz, dz2
4. dxy, dyz, dxz

Number of possible stereoisomers for the complex [Co(en)2Cl2]Cl will be :

1. 3
2. 4
3. 2
4. 1

The coordination number of Co in [Co(en)2Cl2]+ is:

1. 4
2. 3
3. 6
4. 2

Which of the following ligands forms a chelate complex ?

1. Ammonia
2. Water
3. NO2⁻
4. Oxalate ion

According to Werner's theory of coordination compounds :

1. Primary valences are ionisable.
2. Secondary valences are ionisable.
3. Both primary and secondary valences are non-ionisable.
4. Both primary and secondary valences are ionisable.

Which of the following complex ion is not optically active ?

1. [Co(ox)3]3–
2. cis-[Co(en)2Cl2]+
3. trans-[Co(en)2Cl2]+
4. [Co(en)3]3+

Coordination number of Fe in [Fe(C2O4)3]3– is:

1. 6
2. 3
3. 4
4. 5

Which of the following complexes shows geometrical isomerism?

1. [Co(NH3)6]3+
2. [Co(NH3)5Cl]2+
3. [Co(NH3)4Cl2]+
4. [Co(NH3)5(ONO)]2+

Which of the following complexes show linkage isomerism?

1. [Co(NH3)5Cl]2+
2. [Co(NH3)4Cl2]Br2
3. [Co(H2O)6]3+
4. [Co(NH3)5(ONO)]2+

The primary and secondary valences of Co in [Co(en)3]Cl3 respectively are:

1. 3, 3
2. 0, 3
3. 6, 3
4. 3, 6

The number of moles of AgCl precipitated when excess AgNO3 solution is mixed with one mole of [Co(NH3)3Cl3] is :

1. 0
2. 1
3. 2
4. 3

The number of moles of AgCl precipitated when excess AgNO3 solution is mixed with one mole of [Co(NH3)4Cl2]Cl is :

1. 1
2. 0
3. 2
4. 3

The number of moles of AgCl precipitated when excess AgNO3 solution is mixed with one mole of [Co(NH3)6]Cl3 is:

1. 0
2. 3
3. 6
4. 4

Ligand EDTA4− is an example of a:

1. Monodentate ligand
2. Didentate ligand
3. Tridentate ligand
4. Polydentate ligand

Which of the following ligand forms chelate complex?

1. C2O4^2-
2. Cl^-
3. NO2^-
4. NH3

The coordination number of Co in [Co(en)3]^3+ is:

1. 3
2. 4
3. 5
4. 6

Which one of the following complexes is non-ionisable?

1. [Co(NH3)3 Cl3]
2. [Co(NH3)4 Cl2] Cl
3. [Co(NH3)5 Cl] Cl2
4. [Co(NH3)6] Cl3

The type of isomerism shown by the complex [CoCl₂(en)₂]⁺ is:

1. Linkage isomerism
2. Geometrical isomerism
3. Coordination isomerism
4. Ionization isomerism

Which one of the following hybrid states is associated with low spin complex?

1. sp³d
2. sp³
3. sp³d²
4. d²sp³

Which of the following is diamagnetic in nature ? [ Atomic number : Co = 27 ]

1. Co3+, octahedral complex with strong field ligand
2. Co3+, octahedral complex with weak field ligand
3. Co3+, in a square planar complex
4. Co3+, in a tetrahedral complex

Which of the following ligands can show linkage isomerism in a coordination compound?

1. NH3
2. SO4
3. NO2
4. C2O4

On adding AgNO3 solution to 1 mole of complex NiCl2 . 4NH3, two moles of AgCl are formed. The secondary valency of Ni in the complex will be:

1. 4
2. 2
3. 3
4. 6

On adding AgNO₃ solution to 1 mole of CoCl₃.4NH₃, one mole of AgCl is precipitated. The secondary valency of Co is:

1. 6
2. 4
3. 3
4. 7

The compounds [Co(SO4)(NH3)5]Br and [Co(Br)(NH3)5]SO4 represent:

1. optical isomerism
2. linkage isomerism
3. ionisation isomerism
4. coordination isomerism

Assertion (A): Low spin tetrahedral complexes are rarely observed. Reason (R): Crystal field splitting energy is less than pairing energy for tetrahedral complexes. Select the correct answer.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): EDTA is used to determine hardness of water. Reason (R): EDTA is a bidentate ligand.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): Low spin tetrahedral complexes are rarely observed. Reason (R): Crystal field splitting energy is less than pairing energy for tetrahedral complexes.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The oxidation state of Fe in [Fe(CO)5] is

1. +2
2. 0
3. +3
4. +5

The formula of the complex dichloridobis (ethane–1, 2-diamine) platinum (IV) nitrate is

1. [PtCl2(en)2(NO3)2]
2. [PtCl2(en)2](NO3)2
3. [PtCl2(en)2(NO3)]NO3
4. [Pt(en)2(NO3)2]Cl2

What is the secondary valency of Cobalt in [Co(en2)Cl2]+?

1. 6
2. 4
3. 2
4. 8

Which of the following ligands is an ambidentate ligand?

1. CO
2. NO2
3. NH3
4. H2O

The formula of the complex Iron (III) hexacyanidoferrate (II) is:

1. Fe2[Fe(CN)6]3
2. Fe4[Fe(CN)6]3
3. Fe[Fe(CN)6]
4. Fe3[Fe(CN)6]2

How many ions are produced in the solution from the complex [Ni(NH3)6]Cl2?

1. 4
2. 3
3. 2
4. 5

Which of the following species is not expected to be a ligand?

1. CO
2. +4NH
3. NH3
4. H2O

Which of the following is the most stable complex species?

1. [Fe(C2O4)3]3-
2. [Fe(CN)6]3-
3. [Fe(CO)5]
4. [Fe(H2O)6]3+

Optical isomerism is not shown by the complex:

1. [Co(en)2Cl2]+ (trans form)
2. [Co(en)2Cl2]+ (cis form)
3. [Cr(ox)3]3−
4. [Cr(en)3]3+

Which of the following is a polydentate ligand?

1. NH₃
2. H₂N - CH₂ - CH₂ - NH₂
3. EDTA⁴⁻
4. C₂O₄²⁻

Which of the following coordination compounds exhibits linkage isomerism?

1. [Co(NH₃)₃Cl₃]
2. [Co(NH₃)₅(CO₃)]Cl
3. [Co(NH₃)₅NO₂](NO₃)₂
4. [Co(en)₃]Cl₃

[Co(NH3)5NO3]SO4 and [Co(NH3)5SO4]NO3 exhibit:

1. linkage isomerism
2. ionization isomerism
3. optical isomerism
4. coordination isomerism

In which of the following does the central atom exhibit an oxidation state of +3?

1. K2[Ni(CN)4]
2. K4[Fe(CN)6]
3. [Fe(C2O4)3]3-
4. [Cu(NH3)4]2+

What type of isomerism is shown by the following pair of complex compounds? [Co(NH3)6][Cr(CN)6] and [Cr(NH3)6][Co(CN)6]

1. Linkage isomerism
2. Hydrate isomerism
3. Coordination isomerism
4. Ionization isomerism

In which of the following does the central atom exhibit an oxidation state of +4?

1. K2[Ni(CN)4]
2. [Cu(NH3)4]²⁺
3. [Pt(NH3)2Cl2]
4. [Pt(en)2Cl2]²⁺

The compounds [Cr(H₂O)₆]Cl₃, [Cr(H₂O)₅Cl]Cl₂ . H₂O and [Cr(H₂O)₄Cl₂]Cl . 2H₂O exhibit:

1. Linkage isomerism
2. Geometrical isomerism
3. Ionization isomerism
4. Hydrate isomerism

The magnetic moment of [NiCl4]2–

1. 1.82 BM
2. 2.82 BM
3. 4.42 BM
4. 5.46 BM

Assertion (A): Trans [CrCl2(ox)2]3– shows optical isomerism. Reason (R): Optical isomerism is common in octahedral complexes involving didentate ligands.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): EDTA is a hexadentate ligand. Reason (R): EDTA has 2 nitrogen and 4 oxygen donor atoms.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): [Co(NH3)5 SO4] Cl gives a white precipitate with silver nitrate solution. Reason (R): The complex dissociates to give Cl– and SO42– ions.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Define the following terms : (a) Ambidentate ligand (b) Crystal field splitting energy

Write IUPAC names of the following coordination compounds: (i) [Ag(NH3)2][Ag(CN)2] (ii) K3[Fe(C2O4)3]

Define coordination number. Indicate the type of isomerism exhibited by the following complex: [Co(en)3]Cl3

(a) Define didendate ligand. Give an example. (b) Indicate the type of isomerism exhibited by the given complex : [Pt(NH 3)(H2O)Cl2]

(a) Define coordination number. (b) Indicate the type of isomerism exhibited by the following complex: [Co(en)3]Cl3

Write IUPAC names of the following compounds: (i) [PtCl2(en)2]SO4 (ii) (NH4)2[CoF4]

Write IUPAC names of the following compounds: (a) [Cr(NH3)4(ONO)Cl]NO3 (b) Na[Ag(CN)2]

Write the formulas for the following coordination compounds: (a) Mercury(I) tetrathiocyanato-S-cobaltate(III) (b) Dichloridobis (ethane-1,2-diamine) platinum(IV) nitrate

Write IUPAC names of the following compounds: (a) [Ag(NH3)2] [Ag(CN)2] (b) [Co(en)3]2 (SO4)3

PtCl4 . 2KCl doesn't give precipitate of AgCl with AgNO3 solution. Write the structural formula and IUPAC name of the complex.

PdCl2 . 2KCl does not give precipitate of AgCl with AgNO3 solution. Write the structural formula and IUPAC name of the complex.

(a) Write IUPAC names of the following coordination compounds: (i) [CoCl2(en)2]SO4 (ii) K3[Fe(C2O4)3]

(a) Write IUPAC names of the following coordination compounds: (i) [CoCl2(en)2]SO4 (ii) K3[Fe(C2O4)3] OR (b) Differentiate between: (i) Double salt and Complex compound (ii) Didentate ligand and Ambidentate ligand

Write the IUPAC name of the complex [Pt(en)2Cl2]2+. Draw the structure of geometrical isomer of this complex which is optically inactive.

(a) Write the IUPAC name of the complex [Pt(en)2Cl2]2+. Draw the structure of geometrical isomer of this complex which is optically inactive. OR (b) (i) Write the formula of the following coordination compound: Pentaamminecarbonatocobalt(III)chloride (ii) Write the IUPAC name of the linkage isomer of the complex [Co(NH3)5(NO2)]Cl2.

Write the IUPAC names of the following: (i) [Co(NH3)5(ONO)]2+ (ii) K2[NiCl4]

(a) Write the IUPAC names of the following: (i) [Co(NH3)5(ONO)]2+ (ii) K2[NiCl4] OR (b) (i) What is a chelate complex? Give one example. (ii) What are heteroleptic complexes? Give one example.

Write IUPAC names of the following coordination entities: (a) [Co(NH3)4Cl(NO2)]Cl (b) [PtCl2(en)2]2+

Write IUPAC names of the following coordination entities: (a) [Cr(NH3)3(H2O)3]Cl3 (b) K3[Al(C2O4)3]

Write IUPAC names of the following: (a) [Co(en)₂(H₂O)(CN)]²⁺ (b) [Ni(NH₃)₆]Cl₂

(a) Which of the following species cannot act as a ligand? Give reason. OH–, NH4, CH3NH2, H2O

(a) Which of the following species cannot act as a ligand? Give reason. OH–, 4NH, CH3NH2, H2O (b) The complex [Co(NH3)5(NO2)]Cl2 is red in colour. Give IUPAC name of its linkage isomer.

Give reasons : (i) Why are low spin tetrahedral complexes not formed ? (ii) Why is [Co(en)3]3+ complex more stable than [Co(NH3)6]3+ ? (iii) Why are geometrical isomers not possible for tetrahedral complexes having two different types of unidentate ligands coordinated to the central metal ion ?

[Co(NH3)6]3+ is diamagnetic whereas [CoF6]3– is paramagnetic. Justify the statement. [Atomic number of Co = 27]. Write the electronic configuration for d4 ion if Δo > P on the basis of crystal field theory.

(a) [Fe(H2O)6]2+ is paramagnetic whereas [Fe(CO)5] is diamagnetic. Justify the statement. [Atomic number of Fe = 26] (b) On the basis of crystal field theory write the electronic configuration for d4 ion if 0 < P.

(a) Explain why [Fe(H2O)6]3+ is strongly paramagnetic whereas [Fe(CN)6]3– is weakly paramagnetic. [Atomic number of Fe = 26] (b) On the basis of crystal field theory, write the electronic configuration for d5 ion for which 0 < P.

Answer the following questions about the complexes [NiCl4]^2− and [Ni(CN)4]^2−: (i) Write the hybridization involved in each case. (ii) Which of them is the inner orbital complex and which one is the outer orbital complex? (iii) Compare their magnetic behaviour. [Atomic number: Ni = 28]

(a) When a coordination compound CoCl3·6NH3 is mixed with excess of AgNO3 solution, 3 moles of AgCl are precipitated per mole of the compound. Write the structural formula of the complex, IUPAC name, its hybridisation and magnetic behaviour on the basis of valence bond theory.

(a) When a coordination compound CoCl3 . 6NH3 is mixed with excess of AgNO3 solution, 3 moles of AgCl are precipitated per mole of the compound. Write the structural formula of the complex, IUPAC name, its hybridisation and magnetic behaviour on the basis of valence bond theory. OR (b) (i) How many geometrical isomers are possible in each of the following complexes? (I) [Cr(C2O4)3]3– (II) [Co(NH3)3Cl3] (ii) [Co(NH3)6]3+ is an inner orbital complex whereas [Ni(NH3)6]2+ is an outer orbital complex. Why? [Atomic number: Co = 27, Ni = 28] (iii) Write the formula of Wilkinson catalyst and its use.

(a) Write the IUPAC name of the following complex : K3[Cr(C2O4)3]. (b) Differentiate between homoleptic complex and heterolyptic complex. (c) Which type of isomerism is exhibited by the following complex : [Pt(NH3)2Cl2]

(a) A coordination compound CrCl3 . 6H2O is mixed with excess of AgNO3 solution, two moles of AgCl are precipitated per mole of the compound. Write the structural formula of the coordination compound. (b) Write the oxidation state and hybridisation of the central metal in the following complex : [Fe(H2O)6]³⁺ [Atomic number of Fe = 26]. (c) Why is [Ni(H2O)6]²⁺ coloured ? [Atomic number of Ni = 28]

(a) Write the IUPAC name of the given complex: [Co(NH3)4(H2O)Cl] Cl2 (b) Define polydentate ligand. Give an example. (c) Mention the type of isomerism exhibited by the given complex: [Co(en)3]Cl3

(a) A coordination compound CrCl3 . 6H2O is mixed with excess of AgNO3 solution, one mole of AgCl is precipitated per mole of the compound. Write the structural formula of the coordination compound. (b) Write the oxidation state and hybridisation of the central metal in the given complex: [Fe(CN)6]³⁻. [Atomic number: Fe = 26] (c) Why is [Ti(H2O)6]³⁺ coloured? [Atomic number: Ti = 22]

(a) Write the IUPAC name of the given complex: K₂[Zn(OH)₄] (b) Differentiate between a double salt and a complex. (c) Mention the type of isomerism exhibited by the following complex: [Pt(NH₃) (H₂O) Cl₂]

(a) A coordination compound CrCl₃ · 6H₂O is mixed with excess of AgNO₃ solution, three moles of AgCl are precipitated per mole of the compound. Write the structural formula of the coordination compound. (b) Write the oxidation state and hybridisation of the central metal in the given complex: [Cr(NH₃)₆]³⁺. [Atomic number: Cr = 24] (c) Why is [Sc(H₂O)₆]³⁺ colourless?

(a) When a co-ordination compound CoCl3·6NH3 is mixed with excess of AgNO3 solution, 3 moles of AgCl are precipitated per mole of the compound. Write (i) Structural formula of the complex (ii) IUPAC name of the complex (iii) Hybridization of the complex using valence bond theory [Atomic number: Co = 27] OR (b) (i) Write IUPAC name of [Pt(NH3)2Cl(ONO)]. (ii) Why [Co(en)3]3+ is more stable complex than [Co(NH3)6]3+ ? (iii) Predict the hybridization of [Ni(CO)4] on the basis of valence bond theory. [Atomic number : Ni = 28]

(a) What is meant by crystal field splitting energy? For a d4 ion, write the configuration if (i) Δo < P, and (ii) Δo > P. (b) Explain why in tetrahedral coordination entities, low spin configurations are rarely observed.

Based on Valence Bond Theory, explain the geometry and magnetic character of [NiCl4]2–. [Atomic number: Ni = 28] Draw the possible isomers of [Co(en)2Cl2]+.

Write the name and structure of a hexadentate ligand.

(a) Answer the following about the complexes [FeF6]3– and [Fe(CN)6]4– : (i) Write the hybridization involved in each case. (ii) Which of them is the outer orbital complex and which one is the inner orbital complex ? (iii) Compare their magnetic behaviour. [Atomic number : Fe = 26]

(a) Answer the following about the complexes [FeF6]3– and [Fe(CN)6]4–: (i) Write the hybridization involved in each case. (ii) Which of them is the outer orbital complex and which one is the inner orbital complex? (iii) Compare their magnetic behaviour. [Atomic number: Fe = 26] OR (b) (i) What happens to the colour of complex [Ti(H2O)6]3+ when heated gradually? (ii) Write the electronic configuration for d5 ion if o ≪ P. (iii) Write the hybridization and magnetic behaviour of the complex [Ni(CO)4]. [Atomic number: Ni = 28]

(a) Write the formula for the following coordination compound: Potassium tetrahydroxidozincate (II) (b) Arrange the following complexes in the increasing order of conductivity of their solution: [Cr(NH3)5Cl]Cl2, [Cr(NH3)3Cl3], [Cr(NH3)6]Cl3 (c) Identify the type of isomerism exhibited by the following complexes: (i) [Co(NH3)5NO2]2+ (ii) [Co(en)3]Cl3

Draw the geometrical isomers of [Co(en)2Cl2]2+. Which geometrical isomer of [Co(en)2Cl2]2+ is not optically active and why?

Draw the geometrical isomers of [Co(en)2Cl2]2+. Which geometrical isomer of [Co(en)2Cl2]2+ is not optically active and why ? Write the hybridisation and magnetic behaviour of [CoF6]3–. [Given : Atomic number of Co = 27]

(a) Draw the geometrical isomers of [Co(en)2Cl2]2+. Which geometrical isomer of [Co(en)2Cl2]2+ is not optically active and why? (b) Write the hybridisation and magnetic behaviour of [CoF6]3–. [Given: Atomic number of Co = 27]

Answer any three of the following questions: (a) Explain the type of hybridization in [Fe(CN)6]3- on the basis of valence bond theory. (Given: Atomic number of Fe = 26) (b) Draw the geometrical isomers of [PtCl2(en)2]2+ ion. (c) [NiCl4]2- is paramagnetic while [Ni(CO)4] is diamagnetic though both are tetrahedral. Why? (d) Name the type of isomerism when ambidentate ligands are attached to central metal ion. Give one example of ambidentate ligand.

(a) On the basis of crystal field theory write the electronic configuration for d5 ion with a strong field ligand for which ΔO > P.

(b) Explain [Fe(CN)6]3– is an inner orbital complex whereas [FeF6]3– is an outer orbital complex.

(a) On the basis of crystal field theory, write the electronic configuration for d4 with a strong field ligand for which Δ0 > P. (b) A solution of [Ni(H2O)6]2+ is green but a solution of [Ni(CO)4] is colourless. Explain.

Write the hybridisation and magnetic character of the following complexes: (i) [NiCl4]²⁻ (ii) [Co(NH3)6]³⁺ (iii) [FeF6]³⁻ [Atomic number: Ni = 28, Co = 27, Fe = 26]

(i) Write the electronic configuration of d5 on the basis of crystal field splitting theory if Δo < P. (ii) [Fe(CN)6]3 is weakly paramagnetic whereas [Fe(CN)6]4 is diamagnetic. Give reason to support this statement. [Atomic no.: Fe = 26] (iii) Write the number of ions produced from the complex [Co(NH3)6]Cl2 in solution.

(a) (i) Write the electronic configuration of d4 on the basis of crystal field splitting theory, if Δo < P. (ii) [Ni(CN)4]2 with square-planar structure is diamagnetic and [NiCl4]2 with tetrahedral geometry is paramagnetic. Give reason to support the statement. [Atomic number: Ni = 28] (iii) Write the number of ions produced in the solution from the following complex: [PtCl2(NH3)4]Cl2

(a) (i) Write the electronic configuration of d4 on the basis of crystal field splitting theory if Δo > P. (ii) [Co(NH3)6]3+ is an inner orbital complex whereas [Ni(NH3)6]2+ is an outer orbital complex. (Atomic number: Co = 27, Ni = 28) (iii) Write the number of ions produced from the complex [Pt(NH3)6]Cl4 in solution.

(a) (i) Give reasons: (I) [Ni(CO)4] is diamagnetic whereas [NiCl4]2– is paramagnetic. [Atomic number: Ni = 28]

(a)(i)(I) Give reasons: [Ni(CO)4] is diamagnetic whereas [NiCl4]2– is paramagnetic. [Atomic number: Ni = 28]

(a) (i) Give reasons: (I) [Ni(CO)4] is diamagnetic whereas [NiCl4]²⁻ is paramagnetic. [Atomic number: Ni = 28] (II) CO is a stronger complexing agent than NH3. (III) The trans isomer of complex [Co(en)2Cl2]⁺ is optically inactive. (ii) Using Crystal Field theory, write the number of unpaired electrons in octahedral complexes of Fe³⁺ in the presence of: (I) Strong field ligand. (II) Weak field ligand. [Atomic number: Fe = 26]

(a) How is the crystal field splitting energy for octahedral complex (Δo) related to that of tetrahedral complex (Δt)?

Answer any five of the following: (a) How is the crystal field splitting energy for octahedral complex (Δo) related to that of tetrahedral complex (Δt)? (b) Write the IUPAC name of the following complex: [PtCl2(en)2] (NO3)2 (c) Write the geometry and magnetic behaviour of the complex [Ni(CO)4] on the basis of Valency Bond Theory (VBT). (d) What type of isomerism is shown by the complex [Co(NH3)6] [Cr(CN)6]? (e) For the coordination compound on the basis of crystal field theory, write the electronic configuration for d^4 ion if Δo < P. Is the coordination compound a high spin or low spin complex? (f) Out of [Co(NH3)6]^3+ and [Co(NH3)4Cl2]^+, which complex is heteroleptic and why? (g) Draw the structures of optical isomers of [PtCl2(en)2]^2+.

(a) Write the IUPAC name of the complex : [Co(H₂O)(CN)(en)₂]²⁺

Chloroform, in the presence of air and sunlight, produces a poisonous gas known as :

1. Phosgene
2. Phosphine
3. Tear gas
4. Mustard gas

(CH3)3C–OC2H5 on reaction with HI gives

1. (CH3)3C–I and C2H5–I
2. (CH3)3C–OH and C2H5–I
3. (CH3)3C–I and C2H5–OH
4. (CH3)3C–OH and C2H5–OH

Consider the following compounds: Chlorobenzene (I), 2,4,6-trinitrochlorobenzene (II), 2,4-dinitrochlorobenzene (III), 4-nitrochlorobenzene (IV). The correct order of increasing ease of nucleophilic substitution reactions of these compounds is :

1. I < IV < III < II
2. I < III < IV < II
3. II < III < IV < I
4. IV < III < II < I

Oxidation of chloroform by air in the presence of sunlight produces a poisonous gas known as:

1. Mustard gas
2. Tear gas
3. Chlorine gas
4. Phosgene gas

The position of − Br in the compound can be classified as :

1. Vinylic
2. Allylic
3. Benzylic
4. Aryl

Which of the following is not correct for SN1 reaction?

1. Follows first order kinetics
2. Favoured by polar protic solvents
3. Proceeds through the formation of carbocation
4. Results in inversion of configuration

Consider the following reaction and identify A and B : CH3Cl + NaI (in dry acetone) → A + B

1. A = CH3I, B = NaCl
2. A = CH3OH, B = NaCl
3. A = CH3CHO, B = NaCl
4. A = C2H6, B = CH3I

Consider the following reaction and identify A and B: CH3Cl + NaI (dry acetone) → A + B

1. A = CH3I, B = NaCl
2. A = CH3OH, B = NaCl
3. A = CH3CHO, B = NaCl
4. A = C2H6, B = CH3I

The conversion of an alkyl halide into an alcohol by aqueous NaOH is classified as

1. an addition reaction
2. a substitution reaction
3. a dehydrohalogenation reaction
4. a dehydration reaction

The synthesis of alkyl fluoride is best accomplished by

1. Sandmeyer reaction
2. Finkelstein reaction
3. Wurtz reaction
4. Swarts reaction

Assertion (A): (CH3)3C–O–CH3 gives (CH3)3C–I and CH3OH on treatment with HI. Reason (R): The reaction occurs by SN1 mechanism.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): Nucleophilic substitution reaction of chlorobenzene is easier than that of chloroethane. Reason (R): C–Cl bond in chlorobenzene has partial double bond character due to resonance.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Out of 2-Bromobutane, 1-Bromobutane, 2-Bromopropane and 1-Bromopropane, the molecule which is chiral in nature is:

1. 2-Bromobutane
2. 1-Bromobutane
3. 2-Bromopropane
4. 1-Bromopropane

Polyhalogen compounds have wide application in industries and agriculture. DDT is also a very important polyhalogen compound. It is a:

1. greenhouse gas
2. fertilizer
3. biodegradable insecticide
4. non-biodegradable insecticide

Assertion (A): n-Butyl chloride has higher boiling point than n-Butyl bromide. Reason (R): C – Cl bond is more polar than C – Br bond.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following molecules is chiral in nature?

1. 1-chloropropane
2. 2-chloropropane
3. 1-chlorobutane
4. 2-chlorobutane

The treatment of ethyl bromide with alcoholic silver nitrite gives:

1. ethyl nitrite
2. nitroethane
3. nitromethane
4. ethene

Assertion (A): The boiling points of alkyl halides decrease in the order RI > RBr > RCl > RF. Reason (R): The van der Waals forces of attraction decrease in the order RI > RBr > RCl > RF.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following compounds would be hydrolysed by aqueous KOH most easily ?

1. CH2 = CH – Br
2. CH3 – CH2 – Br
3. CH3 – CH – CH3 (with Br)
4. CH2 = CH – CH2 – Br

Which reagents are required for one step conversion of chlorobenzene to toluene?

1. NaNO2 + HCl
2. CH3Cl/Anhydrous AlCl3
3. CH3Cl/Fe, Dark
4. CH3Cl, Na, Dry ether

Which reagents are required for one step conversion of Chlorobenzene to Diphenyl?

1. Chlorobenzene, Na, Dry ether
2. Benzene, Anhydrous AlCl3
3. Chlorobenzene/Fe, Dark
4. NaNO2 + HCl

Which of the following haloalkanes react with aqueous KOH most rapidly by SN1 reaction ?

1. 2-Chlorobutane
2. 1-Bromobutane
3. 2-Bromo-2-Methylpropane
4. 2,2-Dimethyl-1-Chloropropane

The synthesis of alkyl fluoride is best carried out by :

1. Finkelstein reaction
2. Swarts reaction
3. Sandmeyer reaction
4. Wurtz reaction

Which of the following haloalkanes is most reactive towards SN2 reaction?

1. CH3 – CH2 – I
2. CH3 – CH2 – Br
3. CH3 – CH2 – Cl
4. CH3 – CH2 – F

Which of the following alkyl halides will undergo SN1 reaction most readily?

1. (CH3)3CI
2. (CH3)3CCl
3. (CH3)3CBr
4. (CH3)3CF

Assertion (A): p-nitroaniline is a weaker base than p-toluidine. Reason (R): The electron withdrawing effect of NO2 group in p-nitroaniline makes it a weaker base.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

(CH3)2CH O CH3 when treated with HI gives :

1. (CH3)2CH I + CH3OH
2. (CH3)2CH OH + CH3 I
3. (CH3)2CH I + CH3 I
4. (CH3)2CH OH + CH3OH

The synthesis of alkyl fluoride is best obtained from:

1. Free radicals
2. Swartz reaction
3. Sandmeyer reaction
4. Finkelstein reaction

In the reaction R-OH + HCl → R-Cl + H2O (with 2ZnCl2), what is the correct order of reactivity of alcohol?

1. 1 < 2 < 3
2. 1 > 3 > 2
3. 1 > 2 > 3
4. 3 > 1 > 2

In the reaction R—OH + HCl —→ (ZnCl2) R—Cl + H2O, what is the correct order of reactivity of alcohol?

1. 1 < 2 < 3
2. 1 > 3 > 2
3. 1 > 2 > 3
4. 3 > 1 > 2

The species that attacks benzene in following is:

1. Cl
2. AlCl4−
3. AlCl3
4. Cl+

The conversion of an alkyl halide into an alkene by alcoholic KOH is classified as

1. a substitution reaction
2. an addition reaction
3. a dehydrohalogenation reaction
4. a dehydration reaction

Racemisation occurs in

1. SN1 reaction
2. SN2 reaction
3. Neither SN1 nor SN2 reaction
4. SN2 reaction as well as SN1 reaction

Which of the following reactions are feasible?

1. CH3CH2Br + Na+O–C(CH3)3 → CH3CH2–O–C(CH3)3
2. (CH3)3C–Cl + Na+O–CH2CH3 → CH3CH2–O–C(CH3)3
3. Both (a) and (b)
4. Neither (a) nor (b)

Assertion (A): Nucleophilic substitution of iodoethane is easier than chloroethane. Reason (R): Bond enthalpy of C-I bond is less than that of C-Cl bond.

1. Both (A) and (R) are true and (R) is the correct explanation of (A)
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A)
3. (A) is true, but (R) is false
4. (A) is false, but (R) is true

Which of the following belongs to the class of Vinyl halides ?

1. CH2 = CHCH2CH2Cl
2. CH2 = C(Br) – CH3
3. CH2 = CH – CH2 – Br
4. CH ≡ C – Br

Retention of configuration is observed in

1. SN1 reaction
2. SN2 reaction
3. Neither SN1 nor SN2 reaction
4. SN2 reaction as well as SN1 reaction

Assertion (A): Chlorobenzene is resistant to electrophilic substitution reaction. Reason (R): C-Cl bond in chlorobenzene acquires partial double bond characters due to resonance.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3. (A) is true, but (R) is false.
4. (A) is false, but (R) is true.

Auto oxidation of chloroform in air and sunlight produces a poisonous gas known as

1. Tear gas
2. Mustard gas
3. Phosgene gas
4. Chlorine gas

Inversion of configuration occurs in

1. SN2 reaction
2. SN1 reaction
3. Neither SN2 nor SN1 reaction
4. SN1 as well as SN2 reaction

Assertion (A): Chlorobenzene is resistant to nucleophilic substitution reaction at room temperature. Reason (R): C–Cl bond gets weaker due to resonance.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true, but (R) is not the correct explanation of (A).
3. (A) is true, but (R) is false.
4. (A) is false, but (R) is true.

Assertion (A): Nucleophilic substitution of iodoethane is easier than chloroethane. Reason (R): Bond energy of C-Cl bond is less than C-I bond.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following has the highest melting point?

1. o-Dichlorobenzene
2. m-Dichlorobenzene
3. p-Dichlorobenzene
4. All have the same melting point

Benzene diazonium chloride on hydrolysis gives:

1. Phenol
2. Chlorobenzene
3. Benzene
4. Aniline

Which of the following belongs to the class of alkyl halides?

1. CH₂ = CH - Cl
2. CH₂ = CH - CH₂ - CH₂ - Cl
3. CH₂ = CH - Cl|CH - CH₃
4. CH ≡ C - CH₂ - Cl

Reaction of 1-phenyl-2-chloropropane with alcoholic KOH gives mainly:

1. 1-phenylpropene
2. 3-phenylpropene
3. 1-phenylpropan-3-ol
4. 1-phenylpropan-2-ol

Assertion (A): Monobromination of aniline can be conveniently done by protecting the amino group by acetylation. Reason (R): Acetylation decreases the activating effect of the amino group.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following molecules has a chiral centre correctly labelled with an asterisk (*)?

1. CH3C*HBrCH3
2. CH3C*HClCH2Br
3. HOCH2C*H(OH)CH2OH
4. CH3C*Br2CH3

Which of the following would not be a good choice for reducing nitrobenzene to aniline?

1. LiAlH4
2. H2/Ni
3. Fe and HCl
4. Sn and HCl

What happens when : (a) n-butyl chloride is treated with alcoholic KOH ? (b) Chlorobenzene is treated with CH3Cl in the presence of anhydrous AlCl3 ?

Why are haloarenes less reactive towards nucleophilic substitution reaction? Give two reasons.

Draw the structure of the given compound: 4–Bromo–3–methylpent–2–ene. What happens when chloroethane is treated with aqueous potassium hydroxide?

(a) Draw the structure of the given compound : 4–Bromo–3–methylpent–2–ene (b) What happens when chloroethane is treated with aqueous potassium hydroxide ?

For the compound having molecular formula C4H9Br, write: (a) the isomer which is most reactive towards SN1 displacement. (b) the isomer which, on reacting with Na metal in the presence of dry ether, gives 2,5-Dimethylhexane.

Draw the structures of major product(s) in each of the following reactions: (b) CH3CH = C(CH3)2 + HBr

(a) Complete the equation: 2NH₂⁻ + (N⁺Cl₂) + H⁺ → ? (b) How will you convert chlorobenzene to p-chloroaniline?

Draw the structures of product(s) in each of the following reactions: (a) CH3–CH=CH2 with NO2, heat, (b) Cl with Br2, anhydrous AlCl3, then with CH3COCl

Why are haloarenes less reactive towards nucleophilic substitution reaction ? How does the presence of nitro (–NO2) group at ortho- and para-positions in haloarenes increase the reactivity towards nucleophilic substitution reaction ?

(a) Which one of the following pairs of substances undergoes SN1 reaction faster and why? CH₃-CH₂-CH₂-Cl OR CH₂=CH-CH₂-Cl

(a) Which halogen compound in the following pair will react faster in SN2 reactions and why ? CH3CH2I OR CH3CH2Br

Which halogen compound in the following pair will react faster in SN1 reaction and why? Why is the dipole moment of chlorobenzene lower than that of cyclohexyl chloride?

Which halogen compound in the following pair will react faster in SN2 reaction and why?

Identify A, B and C in the following reactions: (a) CH3-CH(OH)-CH3 + PCl5 → A + AgCN → B (b) CH3CH2CH2Cl + KOH (ethanol) → C + HBr

Write the main product formed when: (a) n-Butyl chloride is treated with alc. KOH. (b) 2,4,6-Trinitrochlorobenzene is subjected to hydrolysis.

An alkyl halide (A) of molecular formula C6H13Cl on treatment with alcoholic KOH gives two isomeric alkenes (B) and (C) of molecular formula C6H12. Both alkenes on hydrogenation give 2,3-dimethylbutane. Write the structures of (A), (B) and (C).

Which of the following is an appropriate set of reactants for the preparation of 1-methoxy-4-nitrobenzene and why?

(b) Write equations for: Reaction of chlorobenzene with CH3Cl / anhyd. AlCl3

Why haloarenes are not reactive towards nucleophilic substitution reaction? Give two reasons.

Write two differences between SN1 and SN2 reactions. Out of chlorobenzene and 2,4,6-trinitrochlorobenzene, which one is more reactive towards nucleophilic substitution reactions ?

Compound 'X' with molecular formula C4H9Br reacts with aqueous KOH to give an alcohol. The rate of this reaction depends only on the concentration of the compound 'X'. When an optically active isomer 'Y' of the compound 'X' was treated with aqueous KOH solution, the rate of reaction was found to be dependent on concentration of compound 'Y' and aqueous KOH both. (a) Write down the structural formula of both 'X' and 'Y'. (b) Out of 'X' and 'Y', which one will undergo racemisation and why? (c) Out of 'X' and 'Y', which one will form product with inversion of configuration and why?

(a) Write the IUPAC name of the given compound: CH 3CH(CH3)CH(Br)CH3 (b) Define Racemisation. (c) The boiling points of the alkyl halides with the same alkyl group decrease in the given order: RI > RBr > RC l > RF. Explain the above statement.

Give reasons for the following: (a) Alkyl halides, though polar, yet their solubility in water is very low. (b) p-Dichlorobenzene has higher melting point than those of o- and m-isomers. (c) CH3 – I is more reactive than CH3 – Br towards SN2 reactions.

Answer the following: (a) Which isomer of C4H9Br is most reactive towards SN1 reaction? (b) Predict the alkene that would be formed by dehydrohalogenation of 1-Bromo-1-methylcyclohexane. (c) Although chlorine shows strong –I effect, yet it is ortho- and para-directing in electrophilic aromatic substitution reactions. Why?

(a) Which isomer of C4H9Br is most reactive towards SN1 reaction? (b) Predict the alkene that would be formed by dehydrohalogenation of 1-Bromo-1-methylcyclohexane. (c) Although chlorine shows strong –I effect, yet it is ortho- and para-directing in electrophilic aromatic substitution reactions. Why?

Define Racemization. Out of SN1 and SN2 reactions, which is accompanied by racemization ? Give reason in support of your answer.

(a) Account for the following: (i) Allyl chloride is hydrolysed more readily than n-propyl chloride. (ii) Isocyanides are formed when alkyl halides are treated with silver cyanide. (iii) Methyl chloride reacts faster with OH– ion in SN2 reaction than t-butyl chloride.

Account for the following: (a) The C – Cl bond length in chlorobenzene is shorter than that in methyl chloride. (b) Grignard reagents should be prepared under anhydrous conditions. (c) In case of optically active alkyl halides, SN1 reactions are accompanied by racemisation.

Among the following, which will have inversion of configuration on reaction with aqueous alkali and why? (i) 1-chloropropane OR (ii) 2-chloro-2-methylpropane. Which of the following (A) or (B) will be the major product in the reaction given: CH3 – CH2 – CH(Br) – CH3 + alc. KOH → CH3 – CH2 – CH = CH2 (A) + CH3 – CH = CH – CH3 (B)? Give a suitable reason for your answer.

Haloarenes are less reactive towards nucleophilic substitution reactions.

Write any two differences between SN1 and SN2 reactions. Which of the following compounds would undergo SN1 reaction faster and why ? (choice between two structural compounds)

Write any two differences between SN1 and SN2 reactions. Which of the following compounds would undergo SN1 reaction faster and why? CH2–Cl or CH2–Cl (with benzene ring)

A compound (A) with molecular formula C4H9I which is a primary alkyl halide, reacts with alcoholic KOH to give compound (B). Compound (B) reacts with HI to give (C) which is an isomer of (A). When (A) reacts with Na metal in the presence of dry ether, it gives a compound (D), C8H18, which is different from the compound formed when n-butyl iodide reacts with sodium. Write the structures of (A), (B), (C) and (D). Write the chemical equation when compound (A) is reacted with alcoholic KOH.

(a) Which of the following is an allylic halide? (i) CH3-CH=CH-Br (ii) CH2=CH-CH(Br)-CH3. (b) Out of chlorobenzene and 2,4,6-trinitrochlorobenzene, which is more reactive towards nucleophilic substitution and why? (c) Which isomer of C4H9Cl has the lowest boiling point?

Give reasons for the following: (a) Chlorine is ortho/para directing in electrophilic aromatic substitution reactions, though chlorine is an electron withdrawing group. (b) Racemic mixture is optically inactive. (c) Allyl chloride is hydrolysed more readily than n-propyl chloride.

(a) What type of nucleophilic substitution (SN1 or SN2) occurs in the hydrolysis of 2-Bromobutane to form ()-Butan-2-ol ? Give reason. (b) What happens when chlorobenzene and methyl chloride are treated with sodium metal in dry ether ?

What type of nucleophilic substitution (SN1 or SN2) occurs in the hydrolysis of 2-Bromobutane to form ()-Butan-2-ol? Give reason. OR What happens when chlorobenzene and methyl chloride are treated with sodium metal in dry ether?

What type of nucleophilic substitution (SN1 or SN2) occurs in the hydrolysis of 2-Bromobutane to form ()-Butan-2-ol? Give reason.

Write main product formed when: (a) Methyl chloride is treated with NaI/Acetone. (b) 2,4,6-trinitrochlorobenzene is subjected to hydrolysis. (c) n-Butyl chloride is treated with alcoholic KOH.

Answer any 3 of the following: (a) Which isomer of C5H10 gives a single monochloro compound C5H9Cl in bright sunlight ? (b) Arrange the following compounds in increasing order of reactivity towards SN2 reaction: 2-Bromopentane, 1-Bromopentane, 2-Bromo-2-methylbutane

Account for the following: (a) Benzyl chloride is highly reactive towards SN1 reaction. (b) ()-Butan-2-ol is optically inactive, though it contains a chiral carbon atom. (c) Chloroform is stored in closed dark coloured bottles.

(i) How will you bring about the following conversions: (I) Bromobenzene to 1-phenylethanol (II) Benzene to m-nitroacetophenone (ii) An organic compound with the molecular formula C8H8O forms 2,4-DNP derivative, reduces Tollens' reagent and undergoes Cannizzaro reaction. On vigorous oxidation with acidic or alkaline KMnO4 it gives Benzene-1,2-dicarboxylic acid. Identify the compound and write the products when it undergoes Cannizzaro reaction. (iii) Arrange the following compounds in increasing order of their acid strength: C6H5COOH, O2N–CH2–COOH, CF3–COOH, HCOOH

(a) (i) (I) Which of the following is more reactive towards SN1 reaction : 2-Bromo-2-methylbutane or 1-Bromopentane. (II) What type of halide is present in the following compound : CH3-CH(CH3)-C(=CH2)-Cl. (III) Why is chloroform stored in dark coloured bottles ? (ii) Define the following terms: (I) Ambident Nucleophiles (II) Racemic mixture

(a) (i) (I) Which of the following is more reactive towards SN1 reaction: 2-Bromo-2-methylbutane or 1-Bromopentane (II) What type of halide is present in the following compound: CH₃-CH(CH₃)-C(Cl)=CH₂ (III) Why is chloroform stored in dark coloured bottles? (ii) Define the following terms: (I) Ambident Nucleophiles (II) Racemic mixture

Propan-2-ol on oxidation with CrO3 gives :

1. Propanal
2. Propanoic acid
3. Propene
4. Propanone

Assertion (A) : p-nitrophenol is less acidic than phenol. Reason (R) : Nitro group is an electron-withdrawing group, which stabilises the phenoxide ion.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Aspirin is obtained by acetylation of

1. Phenol
2. Salicylaldehyde
3. 2-Hydroxybenzoic acid
4. Benzoic acid

At low temperature, phenol reacts with dil. HNO3 to yield

1. 2, 4, 6-Trinitrophenol
2. o-Nitrophenol only
3. p-Nitrophenol only
4. ortho-and para-nitrophenol

Assertion (A): The presence of –OH group in phenols directs the incoming group to meta position in the ring. Reason (R): –OH group in phenols activates the aromatic ring towards electrophilic substitution reaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): The presence of –OH group in phenols directs the incoming group to ortho and para positions. Reason (R): –OH group in phenols activates the aromatic ring towards electrophilic substitution reaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following is 'not' true about enantiomers ?

1. They have the same chemical reactivity.
2. They have the same specific rotation.
3. They have the same melting or boiling point.
4. They have the same refractive index.

At low temperature, phenol on reaction with Br2 in CS2 gives

1. 2, 4, 6-Tribromophenol
2. a mixture of ortho-and para-bromophenol
3. ortho-bromophenol only
4. para-bromophenol only

Assertion (A) : The presence of –OH group in phenols directs the incoming group at ortho- and para- positions. Reason (R) : –OH group in phenols deactivates the aromatic ring.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following molecules is chiral in nature?

1. Propan–2–ol
2. Butan–2–ol
3. 1–Bromobutane
4. 2–Bromopropane

Identify the correct increasing order of boiling points of the given compounds:

1. Propan–1–ol < butan–1–ol < butan–2–ol < pentan–1–ol
2. Pentan–1–ol < butan–1–ol < butan–2–ol < Propan–1–ol
3. Propan–1–ol < butan–2–ol < butan–1–ol < pentan–1–ol
4. Butan–1–ol < Butan–2–ol < Propan–1–ol < Pentan–1–ol

The intermediate formed during the slowest step involved in the dehydration of alcohol is:

1. protonated alcohol
2. carbanion
3. free radical
4. carbocation

Assertion (A): Phenol is less acidic than 4-methylphenol. Reason (R): The presence of an electron releasing group in phenol makes it less acidic.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The dehydration of 1º, 2º and 3º alcohols follows the order :

1. 2º > 1º > 3º
2. 3º > 2º > 1º
3. 1º > 2º > 3º
4. 1º > 3º > 2º

Assertion (A): Phenol is more acidic than 4-methylphenol. Reason (R): The presence of an electron releasing group in phenol makes it more acidic.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): Ethers have lower boiling points than the boiling points of alcohols. Reason (R): This is due to the presence of hydrogen bonding in alcohols.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Lucas reagent produces cloudiness immediately with:

1. 2-methyl-1-propanol
2. Butan-2-ol
3. 2-methyl-2-propanol
4. Butan-1-ol

Assertion (A): Alcohols act as Bronsted bases as well as Bronsted acids. Reason (R): It is due to the presence of unshared electron pairs on oxygen atom and presence of polar O–H bond.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Williamson synthesis is an example of :

1. Nucleophilic addition reaction
2. Electrophilic substitution reaction
3. Nucleophilic substitution reaction
4. Electrophilic addition reaction

Assertion (A): Alcohols act as Bronsted bases as well as Bronsted acids. Reason (R): Alcohols react as both nucleophiles and electrophiles.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): (CH3)3 C – O – CH3 gives (CH3)3 C – I and CH3OH on reaction with HI. Reason (R): The reaction occurs by SN1 mechanism.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Primary, secondary and tertiary alcohols can be distinguished by :

1. Lucas test
2. Fehling's test
3. Tollens' test
4. Hinsberg's test

Assertion (A) : p-nitrophenol is more acidic than phenol. Reason (R) : Nitro group is an electron-withdrawing group, it stabilises phenoxide ion by dispersal of negative charge.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The compound which undergoes dehydration most easily is

1. 2-Methylpropan–2–ol
2. Ethanol
3. 2-Methylbutan–2–ol
4. Propan–1–ol

Alkenes are formed by heating alcohols with conc. H2SO4. The first step in the reaction is:

1. formation of carbocation
2. formation of ester
3. protonation of alcohol molecule
4. elimination of water

CH3CH2OH can be converted to CH3CHO by :

1. catalytic hydrogenation
2. treatment with LiAlH4
3. treatment with PCC
4. treatment with KMnO4

Williamson synthesis of preparing unsymmetrical ether is :

1. SN1 reaction
2. SN2 reaction
3. Electrophilic addition reaction
4. Elimination reaction

Assertion (A) : Phenol is strongly acidic as compared to ethanol. Reason (R) : Phenoxide ion is more stable than ethoxide ion.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which by-product is obtained in the manufacture of phenol from cumene?

1. Acetaldehyde
2. Acetone
3. Anisole
4. o-Cresol

Assertion (A): Phenol is less acidic than alcohol. Reason (R): Phenoxide ion is more stable than alkoxide ion.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

During dehydration of alcohol to alkene by heating with conc. H2SO4, the initiation step is:

1. Formation of an ester
2. Formation of carbocation
3. Protonation of alcohol
4. Elimination of water

Assertion (A): The bond angle C – O – C in ethers is slightly greater than tetrahedral angle. Reason (R): This is because of the repulsive interaction between the two bulky alkyl groups.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The reaction R – OH + Na → RO– Na+ + 1/2 H2 (g) suggests that alcohols are :

1. Acidic
2. Basic
3. Neutral
4. Amphoteric

At low temperature, phenol reacts with Br2 in CS2 to form :

1. 2,4,6-tribromophenol
2. p-bromophenol
3. o-and p-bromophenol
4. 2,4-dibromophenol

Assertion (A): A mixture of o-nitrophenol and p-nitrophenol can be separated by steam distillation. Reason (R): o-nitrophenol is steam volatile due to intermolecular hydrogen bonding.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

In the reaction R – OH + HCl → (2ZnCl) RCl + H2O, what is the correct order of reactivity of alcohols ?

1. 1 < 2 < 3
2. 2 < 1 < 3
3. 3 > 1 < 2
4. 1 > 2 > 3

Phenol reacts with Bromine (Br2) water to form :

1. 2,4-dibromophenol
2. 2-bromophenol
3. 2,4,6-tribromophenol
4. 4-bromophenol

Assertion (A): A mixture of o-nitrophenol and p-nitrophenol can be separated by steam distillation. Reason (R): o-nitrophenol is steam volatile due to intramolecular hydrogen bonding.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The reaction OH + NaOH (aq) → O–Na+ + 1/2 H2 (g) suggests that phenol is:

1. Basic
2. Neutral
3. Acidic
4. Amphoteric

Phenol reacts with conc. HNO3 to form:

1. Salicylic acid
2. Picric acid
3. Benzoic acid
4. Phthalic acid

Assertion (A): A mixture of o-nitrophenol and p-nitrophenol can be separated by fractional distillation. Reason (R): o-nitrophenol is steam volatile due to intramolecular hydrogen bonding.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The reaction of an alkyl halide with sodium alkoxide forming ether is known as:

1. Wurtz reaction
2. Reimer-Tiemann reaction
3. Williamson synthesis
4. Kolbe reaction

Decarboxylation of sodium benzoate on heating with soda lime gives:

1. benzene
2. benzoic acid
3. benzaldehyde
4. toluene

Dehydration of tertiary alcohols with Cu at 573 K gives:

1. Alkyne
2. Alkene
3. Aldehyde
4. Ketone

Phenol on reaction with aqueous bromine at room temperature gives:

1. 2-bromophenol
2. 3-bromophenol
3. 4-bromophenol
4. 2,4,6-tribromophenol

Phenol does not undergo nucleophilic substitution reaction easily due to:

1. Partial double bond character of C-OH bond
2. Partial double bond character of C-C bond
3. Acidic nature of phenol
4. Instability of phenoxide ion

Ethanol on heating with conc. H2SO4 at 413 K gives:

1. C2H5OSO3H
2. C2H5 – O – CH3
3. C2H5 – O – C2H5
4. CH2 = CH2

Phenol is less acidic than:

1. ethanol
2. o-nitrophenol
3. o-methoxyphenol
4. o-methylphenol

(CH3)3 C-O-CH3 reacts with HI to give:

1. (CH3)3 C-I + CH3OH
2. (CH3)3 C-I + CH3-I
3. (CH3)3 C-OH + CH3-I
4. (CH3)3 C-OH + CH3OH

(CH₃)₂CH-O-CH₃ reacts with HI to give:

1. (CH₃)₂CH-OH + CH₃-OH
2. (CH₃)₂CH-OH + CH₃-I
3. (CH₃)₂CH-I + CH₃-OH
4. (CH₃)₂CH-I + CH₃-I

A compound (X) with the molecular formula C₃H₈O can be oxidized by strong oxidizing agents to another compound (Y) whose molecular formula is C₃H₆O₂. The compound (X) is:

1. CH₃-CH₂-O-CH₃
2. CH₃-CH(OH)-CH₃
3. CH₃-CH₂-CH₂-OH
4. None of the above

Which one of the following compounds has the lowest pKa value ?

1. p-Cresol
2. p-Nitrophenol
3. m-Nitrophenol
4. 2,4,6-Trinitrophenol

Assertion (A): The boiling point of ethanol is higher than that of dimethyl ether. Reason (R): Ethanol molecules are associated through hydrogen bonding whereas in dimethyl ether, it is not possible.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which one of the following compounds has the highest pKa value?

1. p-Nitrophenol
2. m-Nitrophenol
3. p-Cresol
4. 2,4,6-Trinitrophenol

C6H5 O CH3 when treated with HI gives:

1. C6H5 I + CH3 OH
2. C6H5 OH + CH3 I
3. C6H5 OH + CH3 OH
4. C6H5 I + CH3 I

Assertion (A): The boiling point of ethanol is higher than that of dimethyl ether. Reason (R): Dimethyl ether molecules are associated through hydrogen bonding.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

CH₃ – O – CH₃ when treated with excess HI gives:

1. CH₃OH + CH₃I
2. 2CH₃OH
3. 2CH₃I
4. CH₃I + CH₄

Assertion (A): Phenol on reaction with aqueous NaOH gives sodium phenoxide. Reason (R): This reaction supports the acidic nature of phenol.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): Boiling point of butan-1-ol is higher than that of butan-1-amine. Reason (R): Being more polar, butan-1-ol forms stronger intermolecular hydrogen bonds as compared to butan-1-amine.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): NH2 group is o- and p-directing in electrophilic substitution reactions. Reason (R): Aniline cannot undergo Friedel-Crafts reaction. Select the correct answer.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): Acetylation of aniline gives a monosubstituted product. Reason (R): Activating effect of NHCOCH3 group is more than that of amino group. Select the correct answer.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

In the reaction R−OH + HCl → R−Cl + H₂O (with ZnCl₂), what is the correct order of reactivity of alcohol?

1. 1 < 2 < 3
2. 1 > 3 > 2
3. 1 > 2 > 3
4. 3 > 1 > 2

Which of the following reactions are feasible ?

1. CH3CH2Br + Na+ O–C(CH3)3 → CH3CH2–O – C(CH3)3
2. (CH3)3 C – Cl + Na+ O– CH2CH3 → CH3CH2 – O – C(CH3)3
3. Both (a) and (b)
4. Neither (a) nor (b)

Aspirin is obtained by the acetylation of which of the following compounds?

1. Salicylaldehyde
2. Salicylic acid
3. Acetyl salicylic acid
4. Phenol

Sodium phenoxide when heated with CO2 under pressure, followed by acidification, yields:

1. Sodium benzoate
2. Salicylic acid
3. Salicylaldehyde
4. Benzoic acid

For the conversion of propene into 1-propanol, which of the following reagents and conditions should be used?

1. Conc. H₂SO₄; H₂O and heat
2. B₂H₆; H₂O₂/OH⁻
3. Dilute H₂SO₄
4. H₂O/H⁺

When diethyl ether is heated with excess of HI, it produces:

1. ethanol
2. iodoform
3. methyl iodide
4. ethyl iodide

Which of the following alkenes on acid catalysed hydration gives a tertiary alcohol?

1. 2-Butene
2. 2-Methylpropene
3. Propene
4. 1-Butene

Which of the following alcohols will not undergo oxidation?

1. Butanol
2. Butan-2-ol
3. 2-Methylbutan-2-ol
4. 3-Methylbutan-2-ol

(a) Write the major product in the following reaction: (benzene) + CH3 – Cl Na dry ether ? (b) What happens when 2-Bromobutane is made to react with alcoholic potassium hydroxide?

Explain the mechanism of acid catalysed hydration of ethene.

Write the mechanism of dehydration of ethyl alcohol with conc. H2SO4 at 413 K.

Write the mechanism of dehydration of ethyl alcohol with conc. H2SO4 at 443 K.

(b) What type of deviation is shown by ethanol and acetone mixture ? Give reason. What type of azeotropic mixture is formed by that deviation ?

Account for the following: (i) Phenol is a stronger acid than an alcohol. (ii) The boiling point of alcohols decreases with increase in branching of alkyl chain.

(a) Predict the products of the following reactions: (i) CH₃CH₂OH →(K, 573Cu) (ii) C₆H₅OH →(aq.Br₂) OR (b) Give reasons for the following: (i) p-nitrophenol is more acidic than p-methylphenol. (ii) (CH₃)₃C−Br on reaction with NaOCH₃ gives alkene as the main product and not an ether.

(a) Account for the following: (i) Phenol is a stronger acid than an alcohol. (ii) The boiling point of alcohols decreases with increase in branching of alkyl chain. OR (b) (i) Write the mechanism of the following reaction: CH3CH2OH →(K, 443K) CH2=CH2 + H2O (ii) Write the equation involved in Reimer-Tiemann reaction.

Write the chemical equation involved in the following reactions: (a) Reimer-Tiemann reaction (b) Acetylation of Salicylic acid

Write the chemical equation involved in the following: (a) Kolbe's reaction (b) Williamson synthesis

Give the structures and IUPAC name of the products expected from the following reactions: (b) Reaction of phenol with Br₂(aq).

Write the mechanism of the following reaction: CH2 = CH2 + H2O →(H+) CH3CH2OH

Write the mechanism of acid dehydration of ethanol to yield ethene.

Why is boiling point of o-dichlorobenzene higher than p-dichlorobenzene but melting point of para isomer is higher than ortho isomer?

(b) (i) Complete the reaction with the main product formed: CH3CH2OH (ii) Convert Bromoethane to Propanamine.

(a) For the pair phenol and cyclohexanol: Why is phenol more acidic than cyclohexanol?

(a) Write equations for: Oxidation of chloroform by air and light

For the pair phenol and cyclohexanol, answer the following: (a) Why is phenol more acidic than cyclohexanol? (b) Give one chemical test to distinguish between the two.

Write the reaction involved in the following: (a) Reimer-Tiemann reaction (b) Kolbe's reaction (c) Friedal-Crafts acylation of anisole

Give reasons for the following: (a) Although chlorine is an electron-withdrawing group, yet it is ortho-, para-directing in electrophilic aromatic substitution reactions. (b) Aryl halides cannot be prepared by reacting phenol with concentrated halogen acids or phosphorus halides. (c) Chloroform is stored in closed dark coloured bottles.

How will you obtain the following from benzene diazonium chloride ? Write chemical equations involved: (a) Phenol (b) Iodobenzene (c) p-Aminoazobenzene

(a) Can sodium ethoxide and t-butyl chloride be used for the preparation of t-butyl ethyl ether? Give suitable explanation. Justify your answer by suggesting the appropriate starting material required for preparation of t-butyl ethyl ether. (b) Give the IUPAC name of above mentioned ether.

(a) Can sodium methoxide and t-butyl bromide be used for the preparation of t-butyl methyl ether. Give suitable reason. Justify your answer by suggesting the appropriate starting material if required for the preparation of t-butyl methyl ether. (b) Give the IUPAC name of above mentioned ether.

(a) Can sodium propoxide and t-butyl chloride be used for the preparation of t-butyl propyl ether? Give suitable explanation. Justify your answer by suggesting the appropriate starting material required for the preparation of t-butyl propyl ether. (b) Give the IUPAC name of the above mentioned ether.

(a) Arrange the following compounds in the increasing order of their acidic strength: 3,5-dinitrophenol, 4-methylphenol, phenol, 2,4,6-trinitrophenol. (b) What happens when: (i) Phenol is distilled with Zn dust? (ii) Anisole is treated with HBr? (write equations)

Write the chemical equation for Williamson's synthesis. Give a method to separate o-nitrophenol and p-nitrophenol. Explain the principle involved.

Write the chemical equation for the following: (i) Preparation of phenol from cumene (ii) Nitration of anisole

Compound (A) (C6H12O2) on reduction with LiAlH4 gives two compounds (B) and (C). The compound (B) on oxidation with PCC gives compound (D) which upon treatment with dilute NaOH and subsequent heating gives compound (E). Compound (E) on catalytic hydrogenation gives compound (C). The compound (D) is oxidized further to give compound (F) which is found to be a monobasic acid (Molecular weight = 60). Identify the compounds (A), (B), (C), (D), (E) and (F).

Give the equations of reactions for the preparation of (any three): (a) Phenol from chlorobenzene (b) Salicylaldehyde from phenol (c) 2-Methoxyacetophenone from anisole (d) Picric acid from phenol

Give reasons for the following: (a) Chlorine is ortho/para directing in electrophilic aromatic substitution reactions, though chlorine is an electron withdrawing group. (b) Racemic mixture is optically inactive. (c) Allyl chloride is hydrolysed more readily than n-propyl chloride.

(a) Write the equations of the reactions involved in the following: (i) Reimer-Tiemann reaction (ii) Kolbe reaction (b) Name the reagent used in the bromination of phenol to form 2,4,6-Tribromophenol.

Write the reactions involved in the following: (i) Reimer-Tiemann reaction (ii) Colbe reaction OR Name the reagent used in the bromination of phenol to form 2,4,6-Tribromophenol.

How do you convert the following: (Any three) (a) Phenol to picric acid (b) Propanone to 2-Methylpropan-2-ol (c) Phenol to anisole (d) Propene to Propan-1-ol

How do you convert the following (Any three): (a) Phenol to 2-Hydroxybenzaldehyde (b) Anisole to 2-Methoxyacetophenone (c) Propene to Propan-2-ol (d) Ethanol to Ethanal

Write the mechanism of the following reaction: 2CH3CH2OH + H+/413K → CH3–CH2–O–CH2–CH3 + H2O

Write the mechanism of the following reaction: 2CH3CH2OH →(H+, 413 K) CH3 – CH2 – O – CH2 – CH3 + H2O. Why ortho-nitrophenol is steam volatile while para-nitrophenol is not ?

(a) (i) Write the mechanism of the following reaction: 2CH3CH2OH H+ 413 K → CH3–CH2–O–CH2–CH3 + H2O (ii) Why ortho-nitrophenol is steam volatile while para-nitrophenol is not? OR (b) What happens when (i) Anisole is treated with CH3Cl/anhydrous AlCl3? (ii) Phenol is oxidised with Na2Cr2O7/H+? (iii) (CH3)3C–OH is heated with Cu/573 K? Write chemical equation in support of your answer.

(a) Write the mechanism of the following reaction: CH3-CH2-OH →(K,443H) CH2=CH2 + H2O (b) Write the equation of the reaction for the preparation of phenol from cumene.

Write the mechanism of the following reaction: CH₃-CH₂-OH (K, 443°C) → CH₂ = CH₂ + H₂O

(a) (i) Why is the C – O bond length in phenols less than that in methanol? (ii) Arrange the following in order of increasing boiling point: Ethoxyethane, Butanal, Butanol, n-butane (iii) How can phenol be prepared from anisole? Give reaction.

(a)(i) Why is the C – O bond length in phenols less than that in methanol?

(b) (v) Draw the structure of 'X' in the following reaction : C6H5CH2CH(OH)CH3 + CrO3 → 'X'

An organic compound 'A', with molecular formula C2H6O reacts with active metals such as sodium to give compound 'B' and hydrogen gas. 'A' on treatment with iodine and sodium hydroxide gives 'C' and in presence of H2SO4 at 413 K gives 'D' (C4H10O). 'D' on reaction with excess of HI gives 'E'. Identify 'A', 'B', 'C', 'D' and 'E' and write all the reactions involved.

Which of the following is 'not' true about enantiomers?

1. They have the same chemical reactivity.
2. They have the same specific rotation.
3. They have the same melting or boiling point.
4. They have the same refractive index.

Identify 'X' in the following reaction : CH 3 – CO – CH2 – COO – CH3 + NaBH4 → 'X'

1. CH 3 – CHOH – CH2 – COO – CH3
2. CH3 – CO – CH2 – CH2 – OH
3. CH 3 – CHOH – CH2 – CH2 – OH
4. CH3 – CHOH – CH2 – COOH

Which of the reactions is used in the conversion of a ketone into hydrocarbon ?

1. Reimer-Tiemann reaction
2. Wolff-Kishner reduction
3. Aldol condensation
4. Stephen reaction

Assertion (A) : All aliphatic aldehydes give a positive Fehling's test. Reason (R) : Aliphatic aldehydes are reduced by Fehling's reagent.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

CH3CH2OH can be converted to CH3CHO by:

1. catalytic hydrogenation
2. treatment with LiAlH4
3. treatment with PCC
4. treatment with KMnO4

Which of the following aldehydes will undergo Cannizzaro reaction?

1. CH3 – CH – CHO with CH3 group
2. (CH3)3C CHO
3. CH3 – CH2 – CHO
4. CH3 – CH – CH – CHO with two CH3 groups

CH3CH2CHO and CH3CH2COOH can be distinguished by:

1. Sodium bicarbonate test
2. Hinsberg test
3. Iodoform test
4. Lucas test

Assertion (A): The solubility of aldehydes and ketones in water decreases with increase in size of the alkyl group. Reason (R): Aldehydes and ketones have dipole-dipole interaction.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The formation of cyanohydrin from an aldehyde is an example of:

1. nucleophilic addition
2. electrophilic addition
3. nucleophilic substitution
4. electrophilic substitution

The product formed as a result of reaction of CH3MgBr and CO2 followed by hydrolysis is:

1. CH3CHO
2. CH3COCH3
3. HCOOH
4. CH3COOH

The IUPAC name of the compound with structure showing 3-oxobutanal is:

1. 1-oxobutanal-3-one
2. 1-oxobutanal
3. 3-oxobutanal
4. 3-oxobutanone

Assertion (A): The pKa of O2N-CH2-COOH is lower than that of CH3-COOH. Reason (R): NO2 group shows electron withdrawing effect which increases the acidic character of O2N-CH2-COOH.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Which of the following is the strongest acid?

1. p-Cl-C6H4COOH
2. p-OH-C6H4COOH
3. C6H5COOH
4. p-NO2-C6H4COOH

Which of the following has the highest boiling point?

1. CH3CHO
2. CH3COCl
3. CH3COCH3
4. CH3COOH

The suitable Grignard reagent used for the synthesis of CH3-CH(CH3)-CH2-OH with methanal is:

1. (CH3)2CH-CH2MgBr / H2O
2. CH3MgBr / H2O
3. (CH3)2CHMgBr / H2O
4. CH3CH2CH2MgBr / H2O

Assertion (A): Fluoroacetic acid is stronger acid than chloroacetic acid. Reason (R): This is due to greater electron withdrawing nature of F than Cl.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Aspirin is formed by the acetylation of:

1. Benzoic acid
2. Phenol
3. Salicylic acid
4. Phthalic acid

Which of the following is most reactive in nucleophilic addition reactions?

1. HCHO
2. CH3CHO
3. CH3COCH3
4. CH3COC2H5

Which of the following does not give aldol condensation reaction?

1. CH3–CHO
2. (b)
3. (c)
4. CH3COCH3

Aldehydes and ketones react with hydroxylamine to form

1. hydrazones
2. cyanohydrins
3. semicarbazones
4. Oxime

The reagent that can be used to distinguish acetophenone and benzophenone is

1. 2, 4-dinitrophenyl hydrazine
2. aqueous NaHSO3
3. Fehling solution
4. I2 and NaOH

Which of the following compounds will undergo self-condensation in the presence of dilute NaOH solution?

1. C6H5CHO
2. CH3CH2CHO
3. (CH3)3C–CHO
4. H–CHO

The reactivities of the carbonyl compounds HCHO (I), CH3CHO (II) and CH3COCH3 (III) towards nucleophilic addition reaction decreases in the order:

1. III > II > I
2. I > II > III
3. II > III > I
4. I > III > II

A compound (A) with molecular formula C5H10O, forms a compound on reduction gives n-pentane. The compound (A) is:

1. Pentan-3-one
2. Pentanal
3. Pentanol
4. Pentan-2-one

Which of the following reagents would one choose to transform CH₃COCl into acetone?

1. (CH₃)₂Cd
2. CH₃MgBr
3. CH₃Cl
4. (CH₃O)₂Mg

C6H5CHO + CH3COCH3 →(OH) C6H5CH = CH-COCH3. This reaction is known as:

1. Aldol condensation
2. Cross-Aldol condensation
3. Cannizzaro reaction
4. Friedel-Crafts reaction

This reaction is known as:

1. Cannizzaro reaction
2. Etard reaction
3. Rosenmund reduction
4. Aldol condensation

Which one of the following has lowest pKa value?

1. CH3 – COOH
2. O2N – CH2 – COOH
3. Cl – CH2 – COOH
4. HCOOH

Assertion (A): Acetic acid but not formic acid can be halogenated in presence of red P and Cl2. Reason (R): Acetic acid is a weaker acid than formic acid.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Assertion (A): Bromination of benzoic acid gives m-bromobenzoic acid. Reason (R): Carboxyl group increases the electron density at the meta position.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A)
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A)
3. Assertion (A) is true, but Reason (R) is false
4. Assertion (A) is false, but Reason (R) is true

Which of the following would not be a good choice for reducing nitrobenzene to aniline?

1. LiAlH4
2. H2/Ni
3. Fe and HCl
4. Sn and HCl

Assertion (A): The final product in Aldol condensation is always α-β-unsaturated carbonyl compound. Reason (R): α-β-unsaturated carbonyl compounds are stabilised due to conjugation.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

(a) How can acetaldehyde be prepared from acetyl chloride?

Give a simple chemical test to distinguish between 3-pentanone and 2-pentanone, and write an equation for Clemmensen reduction.

Carboxylic acid is more acidic than phenol. Give reason.

Write the chemical equation when: (a) Butan-2-one is treated with Zn(Hg) and conc. HCl. (b) Two molecules of benzaldehyde are treated with conc. NaOH.

Write the chemical equations when: (a) Pentan-3-one is treated with H2N-NH2 followed by heating with KOH in high boiling solvent such as ethylene glycol. (b) Two molecules of (CH3)3C-CHO are treated with conc. NaOH.

Write the chemical equations when: (a) Ethanal is treated with 2,4-dinitrophenylhydrazine? (b) Propanone is treated with Zn(Hg) and conc. HCl?

Complete and balance the following chemical equations: (a) KMnO4 heat (b) MnO2 + 2C2O4 + 16H+

Write the structures and IUPAC names of the products expected from the following reactions: (a) Reaction of methanal with (CH3)2CHMgBr followed by hydrolysis. (b) Reaction of phenol with conc. HNO3.

Give reasons for the following: (a) Carboxylic carbon is less electrophilic than Carbonyl carbon of aldehydes and ketones. (b) Propanal is more reactive than Propanone towards addition of HCN.

Give the structures and IUPAC name of the products expected from the following reactions: (a) Reaction of methanal with C₆H₅-CH₂-MgBr followed by hydrolysis.

Give reasons: (a) Formic acid is a stronger acid than acetic acid.

Write the products of the following reactions: (i) Reaction with concentrated NaOH. (ii) Reaction with H2N-NH-CO-NH2

Write the products of the following reactions: (i) Benzaldehyde + Concentrated NaOH (ii) Acetophenone + H₂N-NH-CO-NH₂

Predict the products formed when CH3CH2CHO reacts with the following reagents : (Any two) (i) PhMgBr and then H3O+ (ii) LiAlH4 (iii) HCN

Predict the products formed when CH3CHO reacts with the following reagents: (Any two) (i) CH3MgBr and then H3O+ (ii) Zn(Hg)/Conc. HCl (iii) Tollens reagent

Arrange the following compounds in the increasing order of their property indicated: (Any two) (i) Acetaldehyde, Benzaldehyde, Acetophenone, Acetone (Reactivity towards HCN) (ii) (CH3)2CHCOOH, CH3CH2CH(Br)COOH, CH3CH(Br)CH2COOH (Acidic strength) (iii) CH3CH2OH, CH3CHO, CH3COOH (Boiling point)

Write reasons for the following statements: (i) Benzoic acid does not undergo Friedel-Crafts reaction. (ii) Oxidation of aldehydes is easier than that of ketones.

Give reasons for the following statements (Any two): (i) Benzaldehyde is less reactive than propanal in nucleophilic addition reactions. (ii) Carboxylic acids do not give reactions of carbonyl group. (iii) 4-nitrobenzoic acid is a stronger acid than benzoic acid.

(i) (CH3)3C-CHO does not undergo aldol condensation. Why? (ii) Distinguish between Acetophenone and Benzophenone with the help of a chemical test.

How do you convert the following ? (a) Propanone to Propan-2-ol (b) Ethanal to Ethane (c) Sodium benzoate to Benzene

Give reasons for the following: (a) Carboxylic acids have higher boiling point than alcohols of comparable molecular masses. (b) Alpha (α) hydrogens of aldehydes and ketones are acidic in nature. (c) Nucleophilic addition of ammonia and its derivatives does not occur with carbonyl group in strongly acidic medium.

Write the reaction involved in (a) Rosenmund's reduction (b) Cannizzaro's reaction (c) Hell – Volhard – Zelinsky reaction

An organic compound (A) with molecular formula C3H5N on reaction with C6H5MgBr followed by hydrolysis, gives a compound (B). Compound (B) forms an orange-red precipitate with 2,4-DNP reagent and does not give iodoform test. It neither reduces Tollens' or Fehling's reagent nor does it decolourise bromine water. On drastic oxidation with chromic acid it gives a carboxylic acid (C) having molecular formula C7H6O2. Identify the compounds (A), (B) and (C). Write the reactions of compound (A) with C6H5MgBr followed by hydrolysis to give compound (B).

Write the structures of A, B and C in the following reactions:

What happens when: (a) Propanenitrile is treated with phenyl magnesium bromide followed by hydrolysis? (b) p-fluorotoluene is treated with CrO3 in the presence of acetic anhydride followed by hydrolysis with aqueous acid. (c) Phthalic acid is treated with NH3 followed by heating? Write chemical reactions in support of your answer.

How do you convert the following ? (a) Acetophenone to Benzoic acid (b) Acetonitrile to Acetone (c) Benzoic acid to Benzene

How do you convert the following? (a) Toluene to Benzaldehyde (b) Benzoyl chloride to Acetophenone (c) Bromobenzene to Benzoic acid

How do you convert the following? (a) Benzene to m-Nitroacetophenone (b) Bromobenzene to 1-Phenylethanol (c) But-3-en-2-one to Prop-2-en-1-oic acid

(a) (i) Arrange the following compounds in increasing order of their acidic strengths: CH₃CH(Br)CH₂COOH, CH₃CH(CH₃)COOH, CH₃CH₂CH(Br)COOH (ii) Why is CH₃CHO more reactive than acetone towards reaction with HCN? (iii) Complete the equation: CH₃CH=O + NH₂NH₂ → ?

What happens when (a) Ethanal is treated with CH3MgBr followed by hydrolysis ? (b) Phenol is treated with Zinc dust ? (c) Anisole is treated with HI ?

Explain the following reactions : (a) Rosenmund's Reduction (b) Cannizzaro's reaction (c) Hell-Volhard Zelinsky reaction

An aromatic compound 'A' with molecular formula C8H8O gives positive 2,4-DNP test. It gives yellow precipitate of compound 'B' on treatment with sodium hypoiodite. Compound 'A' does not react with Tollen's or Fehling's reagent; on drastic oxidation with KMnO4 it forms a carboxylic acid 'C'. Elucidate the structures of A, B and C. Also give their IUPAC names.

A compound 'A' with molecular formula C4H8O gives positive 2,4-DNP test. It gives yellow precipitate of compound 'B' on treatment with sodium hypoiodite. Compound 'A' does not react with Tollen's or Fehling's reagent; on drastic oxidation with KMnO4, it forms a carboxylic acid 'C'. Elucidate the structures of 'A', 'B' and 'C'. Also give their IUPAC names.

An organic compound 'A' (molecular formula C8H8O) gives 2,4-DNP test. It does not give Tollen's test, but gives a yellow precipitate 'B' with NaOH and I2. On drastic oxidation, it gives a carboxylic acid 'C' with formula C7H6O2. Identify 'A', 'B', 'C' and write the reactions involved.

Write the products formed in the following reaction: CH3CHO + NH2CONHNH2 →

A compound (A) with molecular formula C4H5N on reduction with DIBAL-H followed by hydrolysis, gives a compound (B). Compound (B) gives positive Tollens' test but does not give iodoform test. Compound (B) can also be obtained when ethanal is treated with dilute NaOH followed by heating. Identify (A) and (B). Write the reactions of (A) with DIBAL-H followed by hydrolysis.

Write structure of the products of the following reactions: (a) MgBr + HCHO followed by H+/H2O. (b) An aromatic compound + conc. HNO3. (c) An organic compound + HI followed by OCH3.

Give reasons for the following: (a) Benzoic acid does not undergo Friedel-Crafts reaction. (b) HCHO is more reactive than CH3CHO towards addition of HCN. (c) Vinyl group directly attached with carboxylic acid should decrease the acidity of corresponding carboxylic acid due to resonance, but on the contrary it increases the acidity.

Write structure of the products of the following reactions : (a) 3-OCH3-C6H4-CHO + HI → (b) C6H5-OH + conc. HNO3 → (c) C6H5-MgBr + HCHO → (followed by H+/H2O)

Compound (A) (C6H12O2) on reduction with LiAlH4 gives two compounds (B) and (C). The compound (B) on oxidation with PCC gives compound (D) which upon treatment with dilute NaOH and subsequent heating gives compound (E). Compound (E) on catalytic hydrogenation gives compound (C). The compound (D) is oxidized further to give compound (F) which is found to be a monobasic acid (Molecular weight = 60). Identify the compounds (A), (B), (C), (D), (E) and (F).

Write the reaction involved in the following: (a) Wolff-Kishner reduction (b) Decarboxylation reaction (c) Cannizzaro reaction

How will you bring about the following conversions ? (any three) (a) Benzoic acid to Benzaldehyde (b) Ethanal to Propanone (c) Acetophenone to Benzoic acid (d) Bromobenzene to 1-Phenylethanol

Give the structures of A, B and C in the following reactions:

Explain why: (i) Carboxyl group in benzoic acid is meta directing. (ii) Sodium bisulphite is used for the purification of aldehydes and ketones. (iii) Carboxylic acids do not give characteristic reactions of carbonyl group.

Complete the following reactions:

(a) Explain why: (i) Carboxyl group in benzoic acid is meta directing. (ii) Sodium bisulphite is used for the purification of aldehydes and ketones. (iii) Carboxylic acids do not give characteristic reactions of carbonyl group. OR (b) A compound with molecular formula C₃H₈O on reaction with Cu at 573 K gives a compound B. B gives positive Fehling test and also reacts with iodine and NaOH solution. B does not give iodoform test but C precipitates. Identify A to D.

(a) Explain why: (i) Carboxyl group in benzoic acid is meta directing. (ii) Sodium bisulphite is used for the purification of aldehydes and ketones. (iii) Carboxylic acids do not give characteristic reactions of carbonyl group. OR (b) Give chemical equation for the following reactions: (i) Propanone is treated with dil. Ba(OH)2. (ii) Acetophenone is treated with Zn(Hg)/Conc. HCl. (iii) Benzoyl chloride is hydrogenated in presence of Pd-BaSO4.

Write the equation of the reaction for the preparation of phenol from cumene.

How will you carry out the following conversions (Any two): (i) Propanal to Propane (ii) Ethanal to But-2-enal (iii) Ethanoic acid to ethanamide

Write the equation involved in the following reactions: (i) Rosenmund reduction (ii) Etard reaction (iii) Stephen reaction

Write the equations involved in the following reactions : (i) Cannizzaro reaction (ii) Aldol condensation (iii) Hell-Volhard-Zelinsky reaction

Arrange the following compounds in increasing order of their reactivity towards HCN: CH3CHO, CH3CH2CHO, CH3-C(=O)-CH2-CH3, CH3-C(=O)-CH3

A compound gives yellow precipitate with Iodoform reaction and reacts with HCN to form a compound. On hydrolysis, products A and B are identified. Write equations for the reactions involved.

Give reasons for the following : (i) Oxidation of propanal is easier than propanone. (ii) There are two − NH2 groups in semicarbazide. However, only one − NH2 groups is involved in the formation of semicarbazones. (iii) HCHO does not undergo aldol condensation reaction. (iv) Boiling points of carboxylic acids are higher than those of alcohols of comparable molecular masses. (v) Aldehydes are more reactive towards nucleophilic addition reactions than ketones.

An organic compound (X) has the molecular formula C5H10O. Draw structures for (X) if it: (I) does not give Tollen's test but gives a positive iodoform test. (II) does not give Tollen's test and iodoform test but undergoes Aldol condensation. (III) undergoes Cannizzaro's reaction.

(a) (i) An organic compound (X) has the molecular formula C5H10O. Draw structures for (X) if it: (I) does not give Tollen's test but gives a positive iodoform test. (II) does not give Tollen's test and iodoform test but undergoes Aldol condensation. (III) undergoes Cannizzaro's reaction. (ii) Show how each of the following compounds can be converted to benzoic acid: (I) Acetophenone (II) Ethyl benzene

How will you convert the following: (i) Propanone to Propene (ii) Benzoic acid to Benzaldehyde (iii) Benzene to m-Nitroacetophenone. Arrange the following compounds in increasing order of their reactivity towards HCN. Identify the compounds, which would undergo Aldol condensation.

(a) How will you convert the following : (i) Propanone to Propene (ii) Benzoic acid to Benzaldehyde (iii) Benzene to m-Nitroacetophenone (b) (i) Arrange the following compounds in increasing order of their reactivity towards HCN : CH3 CH3 C = O, (CH3)3 C (CH3)3 C C = O, CH3 H C = O (ii) Identify the compounds, which would undergo Aldol condensation : HCHO, C 6H5CHO, CH3CHO

(a) How will you convert the following: (i) Propanone to Propene (ii) Benzoic acid to Benzaldehyde (iii) Benzene to m-Nitroacetophenone (b) (i) Arrange the following compounds in increasing order of their reactivity towards HCN: (CH3)2C=O, [(CH3)3C]2C=O, CH3CH2CHO (ii) Identify the compounds, which would undergo Aldol condensation: HCHO, C6H5CHO, CH3CHO, (CH3)3CCHO

Write the product(s) when: (I) One mol of ethanal is treated with 1 mol of CH3OH in the presence of dry HCl gas. (II) Benzaldehyde is treated with conc. NaOH. (III) Ethanoic acid is heated in the presence of P2O5. Write a simple chemical test to distinguish between Ethanal and Propanal. Write the name of the reagent to transform Allyl alcohol to Propenal.

(a) (i) Write the product(s) when: (I) One mol of ethanal is treated with 1 mol of CH3OH in the presence of dry HCl gas. (II) Benzaldehyde is treated with conc. NaOH. (III) Ethanoic acid is heated in the presence of P2O5.

(a) Write the product(s) when: (I) One mol of ethanal is treated with 1 mol of CH3OH in the presence of dry HCl gas. (II) Benzaldehyde is treated with conc. NaOH. (III) Ethanoic acid is heated in the presence of P2O5. (ii) Write a simple chemical test to distinguish between Ethanal and Propanal. (iii) Write the name of the reagent to transform Allyl alcohol to Propenal.

(a)(i) How will you bring about the following conversions: (I) Bromobenzene to 1-phenylethanol (II) Benzene to m-nitroacetophenone (ii) An organic compound with the molecular formula C8H8O forms 2,4-DNP derivative, reduces Tollens' reagent and undergoes Cannizzaro reaction. On vigorous oxidation with acidic or alkaline KMnO4 it gives Benzene-1,2-dicarboxylic acid. Identify the compound and write the products when it undergoes Cannizzaro reaction. (iii) Arrange the following compounds in increasing order of their acid strength: C6H5COOH, O2N–CH2–COOH, CF3–COOH, HCOOH

(A) (a) 'A' and 'B' are two functional isomers of compound C4H8O. On heating with NaOH and I2, isomer 'B' forms yellow precipitate of iodoform whereas isomer 'A' does not form any precipitate. (i) Identify 'A' and 'B'. (ii) What happens when isomer 'A' is treated with Zn(Hg) in the presence of Conc. HCl ? (iii) Write the reaction of isomer 'B' with NaOH and I2. (b) Arrange the following in the increasing order of their property as indicated : (i) Ethanol, Ethanoic acid, Ethanal (boiling point). (ii) Ethanal, Methanal, acetone (reactivity towards addition of HCN).

(a) (i) Identify A, B and C in the following reactions: (with structural formulas shown) (ii) Give reasons for the following: (I) Carboxylic acids do not give the characteristic reactions of carbonyl group. (II) Ethanoic acid is a stronger acid than ethanol.

Identify A, B and C in the following reactions: CH3COO⁻ + CrO3 (with K2Cr2O7, H⁺, heat, 273 K, 28 bar) → A + 3H2O → B → C

An organic compound (X) having molecular formula C5H10O can show various properties depending on its structures. Draw each of the structures if it: (I) shows Cannizzaro reaction. (II) reduces Tollens' reagent and has a chiral carbon. (III) gives positive iodoform test. Write the reaction involved in the following: (I) Clemmensen reduction (II) Etard reaction

An organic compound (X) having molecular formula C5H10O can show various properties depending on its structures. Draw each of the structures if it shows Cannizzaro reaction.

(a) (i) An organic compound (X) having molecular formula C5H10O can show various properties depending on its structures. Draw each of the structures if it: (I) shows Cannizzaro reaction. (II) reduces Tollens' reagent and has a chiral carbon. (III) gives positive iodoform test. (ii) Write the reaction involved in the following: (I) Clemmensen reduction (II) Etard reaction

Write the major product(s) in the following reactions:

(a) (i) Carry out the following conversions: (1) Ethanal to But-2-en-1-al (2) Propanoic acid to 2-chloropropanoic acid (ii) An alkene with molecular formula C5H10 on ozonolysis gives compounds A and B. Compound A gives positive Fehling test and also reacts with iodine and NaOH solution. Compound B gives Fehling test but forms iodoform on reaction with I2 and NaOH solution. Identify A, B and the original alkene.

(a) (i) Carry out the following conversions: (1) Ethanal to But-2-en-1-al (2) Propanoic acid to 2-chloropropanoic acid (ii) An alkene with molecular formula C₅H₁₀ on ozonolysis gives a mixture of two compounds. A gives positive Fehling test and also reacts with iodine and NaOH. B does not give Fehling test but forms an iodoform precipitate. Identify A, B and the alkene. OR (b) (i) Distinguish with a suitable chemical test: (1) CH₃COCH₂CH₃ and CH₃CH₂CH₂CHO (2) Ethanal and Ethanoic acid (ii) Write the structure of oxime of acetone. (iii) Identify A to D: CH₃COOH →(PCl₅) A →(4BaSO₄, Pd/H₂) B →(MgBr/ether) C →(LiAlH₄) D

(a) (i) Carry out the following conversions: (1) Ethanal to But-2-en-1-al (2) Propanoic acid to 2-chloropropanoic acid (ii) An alkene with molecular formula C5H10 on ozonolysis gives positive Fehling test and also reacts with iodine and NaOH forms iodoform. Identify the compounds. OR (b) (i) Distinguish with a suitable chemical test: (1) CH3COCH2CH3 and CH3CH2CH2CHO (2) Ethanal and Ethanoic acid (ii) Write the structure of oxime of acetone. (iii) Identify A to D: CH3COOH →(PCl5) A →(BaSO4/Pd/H2) B →(MgBr/CH3I) C →(LiAlH4) D (then H3O+)

(a) (i) An organic compound (X) having molecular formula C5H10O can show various properties depending on its structures. Draw each of the structures if it (1) gives positive iodoform test. (2) shows Cannizzaro reaction. (3) reduces Tollens reagent and has a chiral carbon. (ii) Write the reaction involved in the following: (1) Wolff-Kishner reduction (2) Hell-Volhard-Zelinsky reaction

An organic compound (X) having molecular formula C₅H₁₀O can show various properties depending on its structures. Draw each of the structures if it (1) gives positive iodoform test (2) shows Cannizzaro reaction (3) has a chiral carbon.

(a) Draw structure of the 2,4-dinitrophenylhydrazone of benzaldehyde.

(a) (i) Write the reaction involved in Cannizaro's reaction. (ii) Why are the boiling point of aldehydes and ketones lower than that of corresponding carboxylic acids? (iii) An organic compound 'A' with molecular formula C5H8O2 is reduced to n-pentane with hydrazine followed by heating with NaOH and Glycol. 'A' forms a dioxime with hydroxylamine and gives a positive Iodoform and Tollen's test. Identify 'A' and give its reaction for Iodoform and Tollen's test.

The reaction of ammonia with a large excess of ethyl chloride will give mainly :

1. Ethylamine
2. Tetraethylammonium chloride
3. Triethylamine
4. Diethylamine

Acetamide reacts with Br2 and aqueous KOH to form :

1. Ethanamine
2. Ammonia
3. Methanamine
4. Ethanenitrile

Assertion (A) : Boiling point of propylamine is higher than that of trimethylamine. Reason (R) : In propylamine, intermolecular hydrogen bonding occurs, whereas trimethylamine does not undergo intermolecular hydrogen bonding.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Aniline on direct nitration yields

1. 51%-ortho, 47%-para, 2%-meta derivatives
2. 51%-meta, 47%-ortho, 2%-para derivatives
3. 51%-para, 47%-meta, 2%-ortho derivatives
4. 51%-ortho, 47%-meta, 2%-para derivatives

Benzene diazonium chloride on reaction with phenol in weakly basic medium gives

1. Azobenzene
2. Benzene
3. Chlorobenzene
4. p-hydroxyazobenzene

CH3 – NH2 on reaction with (CH3CO)2O gives

1. CH 3CONH2
2. CH3COONHCH3
3. CH 3 – NH – CO – CH3
4. CH3 – CO – CH2 – NH2

Identify the compound produced by the reduction of Ethanenitrile with Lithium aluminium hydride:

1. Ethylamine
2. Ethanal
3. Propylamine
4. Methylamine

Assertion (A): Aromatic primary amines can be prepared by Gabriel Phthalimide synthesis. Reason (R): Aryl halides do not undergo nucleophilic substitution with the anion formed by phthalimide.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following reagent is used to distinguish between (C2H5)2NH and (C2H5)3N?

1. CHCl3 + KOH
2. C6H5SO2Cl
3. Conc. HCl + ZnCl2
4. NaOH + I2

Assertion (A): Aromatic primary amines cannot be prepared by Gabriel phthalimide synthesis. Reason (R): Gabriel phthalimide synthesis is used for the preparation of primary aliphatic amines.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which reagent is used to distinguish between C2H5NH2 and (C2H5)2NH ?

1. KMnO4
2. CHCl3 + KOH (ethanolic)
3. NaOH + I2
4. Neutral FeCl3

Assertion (A): Aromatic primary amines can easily be prepared by Gabriel phthalimide synthesis. Reason (R): Gabriel phthalimide synthesis is used to prepare only aliphatic primary amines.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which reagent is used to distinguish between primary, secondary and tertiary amines ?

1. C6H5SO2Cl
2. C6H5COCl
3. CHCl3 + ethanolic KOH
4. NaOH + I2

The correct order of decreasing basic strength in aqueous solution of the following is :

1. (C2H5)3N > C2H5NH2 > (C2H5)2NH
2. (C2H5)2NH > C2H5NH2 > (C2H5)3N
3. C2H5NH2 > (C2H5)2NH > (C2H5)3N
4. (C2H5)2NH > (C2H5)3N > C2H5NH2

Assertion (A): Monobromination of aniline can be conveniently done by protecting the amino group by acetylation. Reason (R): Acetylation increases the activation effect of the amino group.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The correct order of decreasing basicities of C2H5NH2, (C2H5)2NH and (C2H5)3N in aqueous solution is:

1. (C2H5)3N > (C2H5)2NH > C2H5NH2
2. (C2H5)2NH > C2H5NH2 > (C2H5)3N
3. C2H5NH2 > (C2H5)2NH > (C2H5)3N
4. (C2H5)2NH > (C2H5)3N > C2H5NH2

In the reaction of NaOBr with amide, the carbonyl carbon is lost as:

1. HCO3–
2. CO3–2
3. CO2
4. CO

Assertion (A): Diazonium salts of aromatic amines are more stable than those of aliphatic amines. Reason (R): Diazonium salts of aliphatic amines undergo resonance.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The correct order of decreasing basic strength of CH3 − NH2, (CH3)2NH and (CH3)3N in aqueous solution is :

1. (CH3)3N > (CH3)2NH > CH3 − NH2
2. CH3 − NH2 > (CH3)2NH > (CH3)3N
3. (CH3)2NH > CH3 − NH2 > (CH3)3N
4. (CH3)2NH > (CH3)3N > CH3 − NH2

Which of the following reagent is used to convert benzene diazonium chloride to benzene ?

1. H2O
2. LiAlH4
3. C2H5OH
4. CuCN

Assertion (A): Diazonium salts of aromatic amines are more stable than those of aliphatic amines. Reason (R): Diazonium salts of aromatic amines undergo resonance.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The correct order of decreasing order of pKb values is:

1. C6H5NH2 > C6H5NHCH3 > C2H5NH2
2. C2H5NH2 > C6H5NH2 > C6H5NHCH3
3. C6H5NH2 > C2H5NH2 > C6H5NHCH3
4. C6H5NHCH3 > C6H5NH2 > C2H5NH2

Assertion (A): Diazonium salts of aromatic amines are less stable than those of aliphatic amines. Reason (R): Diazonium salts of aromatic amines undergo resonance.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Which of the following reagents are used to prepare primary amines by Hoffmann bromamide degradation reaction ? (i) R-CO-NH2 (ii) NaOH (iii) Br2 (iv) CHCl3

1. (i), (ii) and (iv)
2. (i) and (iii)
3. (i), (ii) and (iii)
4. (i), (iii) and (iv)

The major product of carbylamine reaction is :

1. Carboxylic acid
2. Aldehyde
3. Cyanide
4. Isocyanide

The correct formula of Hinsberg's reagent is :

1. C6H5COCl
2. C6H5SO2Cl
3. C6H5CONHCH3
4. C6H5CH2NH2

Consider the following compounds : C2H5NH2, (C2H5)2NH, C6H5CH2NH2, NH3, C6H5NH2. The correct increasing order of the above compounds on the basis of their basic strength is :

1. C6H5NH2 < NH3 < C6H5CH2NH2 < C2H5NH2 < (C2H5)2NH
2. NH3 < C6H5NH2 < C6H5CH2NH2 < C2H5NH2 < (C2H5)2NH
3. C6H5CH2NH2 < (C2H5)2NH < NH3 < C6H5NH2 < C2H5NH2
4. C2H5NH2 < C6H5NH2 < NH3 < C6H5CH2NH2 < (C2H5)2NH

The Gabriel Phthalimide Synthesis is used for the preparation of

1. Secondary amines
2. Primary aromatic amines
3. Tertiary amines
4. Primary aliphatic amines

Hoffmann Bromamide degradation reaction is given by:

1. ArNO2
2. ArNH2
3. ArCONH2
4. ArCH2NH2

Assertion (A): Acetanilide is less basic than aniline. Reason (R): Acetylation of aniline results in decrease of electron density on nitrogen.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

Assertion (A): Acetanilide is more basic than aniline. Reason (R): Acetylation of aniline results in decrease of electron density on nitrogen.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The IUPAC name for CH3 – CH2 – N(CH3) – CH2 – CH2 – CH3 is:

1. N-methylpentan-2-amine
2. N-ethyl-N-methylpropan-1-amine
3. N,N-diethylpropan-1-amine
4. N,N-dimethylpropan-1-amine

In the Hinsberg's method for separation of primary, secondary and tertiary amines, the reagent used is :

1. Nitrous acid
2. CHCl3 + aq. NaOH
3. Benzene sulfonyl chloride
4. HCl / ZnCl2

Which one of the following amines gives an alcohol on reaction with HNO2 ?

1. Aniline
2. C2H5NH2
3. (C2H5)2NH
4. (C2H5)3N

Assertion(A): Boiling point of (CH3)3N is higher than that of CH3CH2CH2NH2. Reason (R) : Hydrogen bonding is more extensive in CH3CH2CH2NH2.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.

The reagent that can be used to convert benzenediazonium chloride to benzene is:

1. Cu/HCl
2. H2O
3. CH3CH2OH
4. CuCN

The gas evolved when methylamine reacts with HNO2 is:

1. NO
2. N2
3. NH3
4. NO2

Assertion (A): Boiling point of (C2H5)2NH is lower than that of n-C4H9NH2. Reason (R): Hydrogen bonding is much more extensive in n-C4H9NH2 as compared to (C2H5)2NH.

1. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
2. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
3. Assertion (A) is true, but Reason (R) is false.
4. Assertion (A) is false, but Reason (R) is true.