For the reaction
`2SO_(2)(g)+O_(2)(g)=2SO_(3)(g)`
`deltaH=-57.2kJmol^(-1)` and `K_(C)=1.7xx10^(16)` ltbr. Which of the following statements is INCORRECT?

Options

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

Answer

C

Explanation

Given `2SO_(2)(g) + O_(2)(g) rarr 2SO_(2)(g)`
`Delta H = -57.2 KJ//mol`
`Kc = 1.7 xx 10^(16)`
A) From `K darr = Ae^(-DeltaH/RTuarr)` as T increases, K decreases
(B) Equilibrium constant is not a affected by change in volume.
(C) Although Kc is large but it doesn’t mean reaction go for completion.
(D) Equilibrium will shift in forward direction as pressure increases.
Hence (C) is incorrect.