Question

The equilibrium constant for the reaction,
$N_2\left(g\right)+O_2\left(g\right)\leftrightharpoons 2NO\left(g\right)$ is $4.0\times {10}^{-4}$ at $2000K$. In the presence of a catalyst the equilibrium is attained ten times faster. Therefore, the equilibrium constant in presence of the catalyst at $2000K$ is:

• A. $4\times {10}^{-4}$
• B. $40\times {10}^{-4}$
• C. $4\times {10}^{-2}$
• D. Difficult to compute without more data

Answer 1

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

Explanation:

Equilibrium constants are not changed if you add a catalyst. The only thing that changes an equilibrium constant is a change of temperature. The position of equilibrium is not changed if you add a catalyst. A catalyst speeds up both the forward and back reactions by the same amount.

$\therefore$ the equilibrium is the same as without catalyst and with catalyst.

Hence the correct answer is option A