Equilibrium Constant (Kc) Practice Questions with Answers

1. Concept Explanation

The Equilibrium Constant (Kc) is a numerical value that describes the ratio of product concentrations to reactant concentrations for a chemical reaction at equilibrium at a specific temperature. This value is derived from the law of mass action, which states that for a reversible chemical reaction, the rate of the forward reaction is proportional to the product of the active masses of the reactants. When a system reaches equilibrium, the concentrations of products and reactants remain constant over time, though the molecules continue to react. Understanding Kc is essential for predicting the direction of a reaction and the extent to which it will proceed. This concept is closely related to other thermodynamic properties, such as those explored in Heat of Reaction Practice Questions with Answers.

For a generalized reversible reaction:

aA + bB ⇌ cC + dD

The expression for the equilibrium constant Kc is written as:

Formula	Components
Kc = [C]c[D]d / [A]a[B]b	[X] = Molar concentration (mol/L) Exponents (a, b, c, d) = Stoichiometric coefficients Solids (s) and pure liquids (l) are omitted (value = 1)

A high Kc value (Kc > 1) indicates that at equilibrium, the products are favored, while a low Kc value (Kc < 1) suggests that the reactants are favored. If you are also studying acid-base equilibria, you might find Ka and Kb Calculations Practice Questions with Answers helpful for understanding specific types of equilibrium constants. For more in-depth study of chemical principles, resources like Wikipedia's Equilibrium Constant page or Khan Academy's Chemistry modules offer excellent foundational knowledge.

2. Solved Examples

Example 1: Writing the Kc Expression
Write the equilibrium constant expression for the following reaction: 2NOCl(g) ⇌ 2NO(g) + Cl₂(g).

1. Identify the products and reactants. Products: NO and Cl₂. Reactants: NOCl.
2. Determine the coefficients: NO has 2, Cl₂ has 1, and NOCl has 2.
3. Place products in the numerator and reactants in the denominator, raising each to the power of its coefficient.
4. Result: Kc = [NO]²[Cl₂] / [NOCl]²

Example 2: Calculating Kc from Equilibrium Concentrations
For the reaction H₂(g) + I₂(g) ⇌ 2HI(g), the equilibrium concentrations are [H₂] = 0.10 M, [I₂] = 0.20 M, and [HI] = 1.0 M. Calculate Kc.

1. Write the expression: Kc = [HI]² / ([H₂][I₂]).
2. Substitute the values: Kc = (1.0)² / (0.10 × 0.20).
3. Solve the math: Kc = 1.0 / 0.02 = 50.

Example 3: Reaction with a Solid
Write the Kc expression for CaCO₃(s) ⇌ CaO(s) + CO₂(g).

1. Identify the states of matter. CaCO₃ and CaO are solids.
2. Exclude solids from the expression, treating them as 1.
3. Kc = [CaO][CO₂] / [CaCO₃] simplifies to Kc = (1)[CO₂] / (1).
4. Result: Kc = [CO₂]

3. Practice Questions

1. Write the Kc expression for the synthesis of ammonia: N₂(g) + 3H₂(g) ⇌ 2NH₃(g).
2. At a certain temperature, the equilibrium concentrations for the reaction A(g) + B(g) ⇌ C(g) are [A] = 0.5 M, [B] = 0.2 M, and [C] = 2.0 M. Calculate Kc.
3. Determine the Kc expression for the reaction: 2H₂O(l) ⇌ 2H₂(g) + O₂(g).

4. If Kc for 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) is 4.0, what is the Kc for the reverse reaction: 2SO₃(g) ⇌ 2SO₂(g) + O₂(g)?
5. For the reaction PCl₅(g) ⇌ PCl₃(g) + Cl₂(g), the equilibrium concentrations are [PCl₅] = 0.04 M, [PCl₃] = 0.2 M, and [Cl₂] = 0.2 M. Calculate Kc.
6. Write the equilibrium expression for: C(s) + CO₂(g) ⇌ 2CO(g).
7. If Kc = 100 for a reaction, are the products or reactants favored at equilibrium?
8. A reaction 2A(g) ⇌ B(g) has Kc = 0.5. If the equilibrium concentration of A is 2.0 M, what is the concentration of B?
9. How does increasing the temperature affect Kc for an exothermic reaction? (Refer to Le Chatelier's Principle).
10. Write the Kc expression for: AgCl(s) ⇌ Ag⁺(aq) + Cl^-(aq).

4. Answers & Explanations

1. Kc = [NH₃]² / ([N₂][H₂]³). The products are in the numerator and reactants in the denominator, each raised to the power of their stoichiometric coefficients.
2. 20. Kc = [C] / ([A][B]) = 2.0 / (0.5 × 0.2) = 2.0 / 0.1 = 20.
3. Kc = [H₂]²[O₂]. Because H₂O is a pure liquid, it is omitted from the expression.
4. 0.25. The Kc for a reverse reaction is the reciprocal of the forward reaction's Kc (1 / 4.0 = 0.25).
5. 1.0. Kc = ([PCl₃][Cl₂]) / [PCl₅] = (0.2 × 0.2) / 0.04 = 0.04 / 0.04 = 1.0.
6. Kc = [CO]² / [CO₂]. Carbon (C) is a solid and is excluded.
7. Products are favored. Since Kc > 1, the concentration of products is higher than that of reactants at equilibrium.
8. 2.0 M. Kc = [B] / [A]². 0.5 = [B] / (2.0)². 0.5 = [B] / 4. [B] = 0.5 × 4 = 2.0 M.
9. Kc decreases. For an exothermic reaction, heat is a product. Increasing temperature shifts the equilibrium toward the reactants, decreasing the value of Kc. This is a key concept when calculating Enthalpy Change Practice Questions with Answers.
10. Kc = [Ag⁺][Cl^-]. AgCl is a solid and is excluded from the expression.

5. Quick Quiz

6. Frequently Asked Questions

What is the difference between Kc and Kp?

Kc is the equilibrium constant expressed in terms of molar concentrations (mol/L), while Kp is expressed in terms of partial pressures of gases. They are related by the equation Kp = Kc(RT)^Δn, where Δn is the change in moles of gas.

Can Kc ever be a negative value?

No, Kc cannot be negative because it is calculated using concentrations and coefficients, which are always positive or zero. A value of zero would imply no products have formed.

Does a catalyst change the value of Kc?

A catalyst does not change the value of Kc or the position of equilibrium. It only speeds up the rate at which equilibrium is reached by lowering the activation energy for both the forward and reverse reactions.

Why are solids and liquids omitted from Kc?

The concentrations of pure solids and liquids are essentially constant regardless of how much of the substance is present. Therefore, their activity is defined as 1 and they do not affect the ratio in the equilibrium expression.

How is Kc affected by pressure changes?

Kc is only dependent on temperature; changes in pressure or volume may shift the position of equilibrium according to Le Chatelier's principle, but the numerical value of Kc remains the same.

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