Question

For the reaction, \[ 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g), \] \[ \Delta H = -57.2 \, \text{kJ/mol} \quad \text{and} \quad K_c = 1.7 \times 10^{16} \] Which of the following statement is INCORRECT?

• A. The equilibrium constant is large, suggestive of reaction going to completion and so no catalyst is required.
• B. The equilibrium will shift in forward direction as the pressure increases.
• C. The equilibrium constant decreases as the temperature increases.
• D. The addition of inert gas at constant volume will not affect the equilibrium constant.

Hint:

A catalyst speeds up a reaction by lowering the activation energy but does not affect the equilibrium constant.

Answer 1

The Correct Option is A

A large equilibrium constant does suggest that the reaction favors the formation of products. However, catalysts are needed to increase the rate of achieving equilibrium, not to shift the equilibrium. Thus, option (1) is incorrect.

Step 2: Conclusion.
Thus, the correct answer is (1).