Question

For the reaction,
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO3(g),$
$ \Delta H = -57.2\,kJ \; mol^{-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 increase
• 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

Answer: (A)

In option (2)- $\Delta n_g$ is -ve therfore increase in pressure will bring reaction in forward direction.
In option (3)- as the reaction is exothermic therefore increase in temperature will decrease the equilibrium constant.
In option (4)- Equillibrium constant changes only with temperature.
Hence, option (2), (3) and (4) are correct therefore option (1) is incorrect choice.