Question

For the reaction,$2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3;\Delta H=-57.2kJmo{l}^{-1}and{K}_C=1.7\times {10}^{16}$
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

Answer 1

The correct option is A The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required

In option (B): $\Delta n_g$ is -ve, therefore, the increase in pressure will bring reaction in the forward direction.

In option (C): as the reaction is exothermic therefore increase in temperature will decrease the equilibrium constant.

In option (D): Equilibrium constant changes only with temperature.

Hence, option (B), (C) and (D) are correct therefore option (A) is the incorrect choice.