Chemical Equilibrium Class 11 MCQs

(1) Find the conjugate acid of NH₂^–

[A] NH₃

[B] NH₄OH

[C] NH₄⁺

[D] NH₂^–

Answer: NH₃

(2) On increasing the concentration of reactants in a reversible reaction, then equilibrium constant will

[A] depend on the concentration

[B] increase

[C] unchanged

[D] decrease

Answer: unchanged

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(3) Find the increase in equilibrium concentration of Fe³⁺ ions if OH^– ions concentration decreases to 1/4th in the following reaction

[A] 8 times

[B] 16 times

[C] 4 times

[D] 64 times

Answer: 64 times

(4) What will be the pH of a buffer solution having an equal concentration of B^– and HB (K_b = 10^-10 for B^–)

[A] 7

[B] 4

[C] 10

[D] 6

Answer: 4

(5) The equilibrium constant is 278 for the reaction

at the same temperature, what will be the equilibrium constant for the following reaction?

[A] 6 x 10^-2

[B] 1.8 x 10^-3

[C] 1.3 x 10^-5

[D] 3.6 x 10^-5

Answer: 6 x 10^-2

(6) Highest pH will be recorded for which of the following solutions if they are equimolar

[A] AlCl₃

[B] BaCl₂

[C] BeCl₂

[D] LiCl

Answer: BaCl₂

(7) Find the equilibrium constant of the reaction

If the equilibrium constant for the following reactions are given

[A] K₂K₃/K₁

[B] K₁K₃³/K₂

[C] K₂K₃³/K₁

[D] K₂³K₃/K₁

Answer: K₂K₃³/K₁

(8) In 0.10 M aqueous solution of pyridine (C₅H₅N), find the percentage of pyridine that forms pyridinium ion (C₅H₅N⁺H) (K_b for C₅H₅N = 1.7 x 10^-9 )

[A] 1.6%

[B] 0.77%

[C] 0.0060%

[D] 0.013%

Answer: 0.013%

(9) Which of the following aqueous solution will be the best conductor of electricity?

[A] NH₃

[B] CH₃COOH

[C] HCl

[D] C₆H₁₂O₆

Answer: HCl

(10) Find the pH of a solution when 0.01 M HCl and 0.1 M NaOH are mixed in equal volumes

[A] 12.65

[B] 1.04

[C] 7.0

[D] 2.0

Answer: 12.65

(11) At a particular temperature and atmospheric pressure, the solid and liquid phases of a pure substance can exist in equilibrium. Which of the following Does the term define this temperature?

[A] Normal melting point

[B] Equilibrium temperature

[C] Boiling point

[D] Freezing point

Answer: A, D

(12) For the reaction N2O4 (g) ⇌ 2NO2 (g), the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is correct?

[A] The reaction is endothermic

[B] The reaction is exothermic

[C] If NO2 (g) and N2O4 (g) are mixed at 400 K at partial pressures 20 bar and 2 bar respectively, more N2O4 (g) will be formed.

[D] The entropy of the system increases.

Answer: A, C, D

(13) In which of the following reactions, the equilibrium remains unaffected on addition of small amount of argon at constant volume?

[A] H2 (g) + I2 (g) ⇌ 2HI (g)

[B] PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)

[C] N2 (g) + 3H2 (g) ⇌ 2NH3 (g)

[D] The equilibrium will remain unaffected in all the three cases.

Answer: The equilibrium will remain unaffected in all the three cases.

(14) At 500 K, the equilibrium constant, 6Kc, for the following reaction is 5.

1/2 H2 (g) +1/2 I2 (g) ⇌ HI (g)

What would be the equilibrium constant Kc for the reaction 2HI (g) ⇌ H2 (g) + I2 (g)

[A] 0.04

[B] 0.4

[C] 25

[D] 2.5

Answer: 0.04

(15) What will be the correct order of vapour pressure of water, acetone and ether at 30°C. Given that among these compounds, water has a maximum boiling Do point and ether have a minimum boiling point?

[A] Water < ether < acetone

[B] Water < acetone < ether

[C] Ether < acetone < water

[D] Acetone < ether < water

Answer: Water < acetone < ether

(16) On increasing the pressure, in which direction will the gas-phase reaction proceed to re-establish equilibrium, is predicted by applying Le Chatelier’s principle. Consider the reaction.

N2 (g) + 3H2 (g) ⇌ 2NH3 (g)

Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?

[A] K will remain the same

[B] K will decrease

[C] K will increase

[D] K will increase initially and decrease when pressure is very high

Answer: K will remain the same

(17) Which of the following options will be correct for the stage of half completion of the reaction A ⇌ B

[A] ∆Gᶱ= 0

[B] ∆Gᶱ > 0

[C] ∆Gᶱ< 0

[D] ∆Gᶱ= –RT ln2.

Answer: ∆Gᶱ= 0

(18) Ka for CH3COOH is 1.8 × 10–5 and Kb for NH4OH is 1.8 × 10–5. The pH of ammonium acetate will be

[A] 7.005

[B] 4.75

[C] 7.0

[D] Between 6 and 7

Answer: 7.0

(19) What will be the value of pH of 0.01 mol dm–3 CH3COOH (Ka = 1.74 × 10–5 )?

[A] 3.4

[B] 3.6

[C] 3.9

[D] 3.0

Answer: 3.4

(20) In which of the following solvents is silver chloride most soluble?

[A] 0.1 mol dm–3 AgNO3 solution

[B] 0.1 mol dm–3 HCl solution

[C] H2O

[D] Aqueous ammonia

Answer: Aqueous ammonia

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