Question

The equilibrium constant for the reaction, $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$ is $4\times {10}^{-4}$ at $2000K$. In presence of a catalyst, the equilibrium is attained $10$ times faster. Therefore, the equilibrium constant in the presence of the catalyst at $2000K$ is:

• A. $4\times {10}^{-5}$
• B. $4\times {10}^{-4}$
• C. $4\times {10}^{-3}$
• D. $2\times {10}^{-4}$

Answer 1

Answer: (B)

$4\times {10}^{-4}$

The equilibrium constant in the presence of the catalyst at $2000K$ is $4\times {10}^{-4}$.

$K_p$ and $K_c$ values do not change with catalyst. They only change with temperature.

With catalyst equilibrium is attained faster.

Hence, the value of equilibrium constant remains the same.