Question

The equilibrium constant for the reaction $N_{2\left(g\right)}+O_{2\left(g\right)}\rightleftharpoons 2N{O}_{\left(g\right)}$ is $4\times {10}^{-4}$ at 2000 K. In the presence of a catalyst the equilibrium is attained ten times faster. Therefore, the equilibrium constant in presence in catalyst of 2000 K is:

• A. $40\times {10}^{-4}$
• B. $4\times {10}^{-2}$
• C. $4\times {10}^{-3}$
• D. $4\times {10}^{-4}$

Answer 1

The correct option is D $4\times {10}^{-4}$

The value of the equilbrium constant is unaffected by the addition of a catalyst. Both forward and backward reaction rates are affected equally.