The equilibrium constant for the reaction N2(g) + O2(g) → 2NO(g) is 4 × 10–4 at 200 K. In the presence of a catalyst the equilibrium is attained 10 times faster. Therefore the equilibrium constant in presence of the catalyst at 200 K is

Q: The equilibrium constant for the reaction

N2(g) + O2(g) $ \rightleftharpoons $ 2NO(g) is 4 × 10–4 at 200 K. In the presence of a catalyst the equilibrium is attained 10 times faster. Therefore the equilibrium constant in presence of the catalyst at 200 K is

(A) 4 × 10–3

(B) 4 × 10–-4

(C) 4 × 10–5

(D) None

Solution:  Equilibrium constant of a reaction remains unchanged when the same reaction remains unchanged when  the same reaction is carried out in presence of a catalyst because  the catalyst will catalyse both the forward and backward reactions equally.

Abs: (B)