Question

The equilibrium constant for the reaction, $N_2\left(g\right)+O_2\left(g\right)=2NO\left(g\right)$ 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 the presence of the catalyst of $2000$ k is:

• A. $4\times {10}^{-2}$
• B. $40\times {10}^{-4}$
• C. $4\times {10}^{-4}$
• D. $4\times {10}^{-1}$

Answer 1

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

Therefore the equilibrium constant in the presence of a catalyst at 2000 K is same as the equilibrium constant in the absence of catalyst at 2000 K. It is $4\times {10}^{-4}$.

The presence of catalyst does not affect the value of the equilibrium constant. It only increases the rates of forward and reverse reaction to equal extent.