Question

The chemical reaction of a gas phase is given below. \[ 2A(g) + B(g) \rightleftharpoons C(g) + D(g) \] Which one of the following changes will affect the value of \(K_c\)?

• A. Addition of inert gas
• B. Increasing in temperature
• C. Addition of reactants
• D. Addition of catalyst

Hint:

\(K_c\) is constant for a given reaction at a given temperature. Only temperature can change its value.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept:
The equilibrium constant \(K_c\) is a function of temperature only, for a given reaction.

Step 2: Detailed Explanation:
• (A) Addition of inert gas at constant volume does not change the equilibrium constant or the equilibrium position if the volume is constant. • (B) Increasing temperature changes the value of \(K_c\) according to the endothermic or exothermic nature of the reaction. • (C) Addition of reactants changes the equilibrium position but not the value of \(K_c\) (at constant temperature). • (D) A catalyst speeds up the attainment of equilibrium but does not change the value of \(K_c\).

Step 3: Final Answer:
Only a change in temperature affects the value of \(K_c\), which corresponds to option (B).