Chapter 6: Equilibrium MCQs | chemistry Class 11 CBSE

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Chapter 6: Equilibrium MCQs | chemistry Class 11 CBSE | ByteNotes.in

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Question 1

Objective

Which of the following best describes a system at dynamic equilibrium?

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Medium

Question 2

Objective

For the reaction H2(g) + I2(g) ⇌ 2HI(g) at 731 K, if Kc = 46.4, what is Kc for the reaction ½H2(g) + ½I2(g) ⇌ HI(g)?

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Medium

Question 3

Objective

The equilibrium constant Kp for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) is related to Kc by which expression?

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Question 4

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Which of the following correctly represents the equilibrium constant expression for the reaction CaCO3(s) ⇌ CaO(s) + CO2(g)?

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Easy

Question 5

Objective

If Qc < Kc for a reversible reaction, the reaction will:

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Easy

Question 6

Objective

Le Chatelier's principle states that when a system at equilibrium is disturbed, it will:

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Medium

Question 7

Objective

For the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g), increasing pressure at constant temperature will:

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Medium

Question 8

Objective

A catalyst added to a reversible reaction at equilibrium will:

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Medium

Question 9

Objective

According to Brønsted-Lowry theory, which of the following is the conjugate base of H2SO4?

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Question 10

Objective

Which of the following species acts as a Lewis acid?

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Easy

Question 11

Objective

The ionic product of water Kw at 298 K is 1.0 × 10−14. What is the pH of pure water at 298 K?

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Easy

Question 12

Objective

The pH of a 0.01 M solution of HCl at 298 K is:

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Medium

Question 13

Objective

For a weak acid HA with Ka = 1.0 × 10−5 and initial concentration 0.1 M, the approximate degree of ionization is:

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Easy

Question 14

Objective

The relationship between Ka and Kb for a conjugate acid-base pair at 298 K is:

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Easy

Question 15

Objective

A solution of CH3COONa in water is:

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Medium

Question 16

Objective

Buffer solutions resist changes in pH because they:

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Medium

Question 17

Objective

The solubility product Ksp of AgCl at 298 K is 1.8 × 10−10. Its molar solubility in pure water is:

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Medium

Question 18

Objective

If the equilibrium constant for a reaction is Kc = 2 × 10−30, which statement is correct?

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Medium

Question 19

Objective

The Henderson-Hasselbalch equation for an acidic buffer is:

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Easy

Question 20

Objective

Henry's law states that the mass of gas dissolved in a given mass of solvent at any temperature is:

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Chapter 6: Equilibrium | MCQs

Which of the following best describes a system at dynamic equilibrium?

For the reaction H2(g) + I2(g) ⇌ 2HI(g) at 731 K, if Kc = 46.4, what is Kc for the reaction ½H2(g) + ½I2(g) ⇌ HI(g)?

The equilibrium constant Kp for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) is related to Kc by which expression?

Which of the following correctly represents the equilibrium constant expression for the reaction CaCO3(s) ⇌ CaO(s) + CO2(g)?

If Qc < Kc for a reversible reaction, the reaction will:

Le Chatelier's principle states that when a system at equilibrium is disturbed, it will:

For the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g), increasing pressure at constant temperature will:

A catalyst added to a reversible reaction at equilibrium will:

According to Brønsted-Lowry theory, which of the following is the conjugate base of H2SO4?

Which of the following species acts as a Lewis acid?

The ionic product of water Kw at 298 K is 1.0 × 10−14. What is the pH of pure water at 298 K?

The pH of a 0.01 M solution of HCl at 298 K is:

For a weak acid HA with Ka = 1.0 × 10−5 and initial concentration 0.1 M, the approximate degree of ionization is:

The relationship between Ka and Kb for a conjugate acid-base pair at 298 K is:

A solution of CH3COONa in water is:

Buffer solutions resist changes in pH because they:

The solubility product Ksp of AgCl at 298 K is 1.8 × 10−10. Its molar solubility in pure water is:

If the equilibrium constant for a reaction is Kc = 2 × 10−30, which statement is correct?

The Henderson-Hasselbalch equation for an acidic buffer is:

Henry's law states that the mass of gas dissolved in a given mass of solvent at any temperature is:

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