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

Q: The equilibrium constant for the reaction $ N_2(s) + O_2(g) \rightleftharpoons 2 NO(g) $ is 4 × 10–4 at 200 K. In presence of a catalyst the equilibrium is attained 10 times faster. Therefore, the equilibrium constant in presence of catalyst at 200 K is

(A) 40 × 10–4

(B) 4 × 10–4

(C) 4 × 10–3

(D) Can’t be calculated

Solution: Kp and KC value doesn’t depend on catalyst

Ans: (B)