Question

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

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

Answer 1

Answer: (D)

$\because K=\frac{[\text{ conc. of product }]}{[\text{ conc. of reactant }]}$

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

Qn adding catalyst. the equilibrium attain 10 time factor.

As equilibrium constant depends on temperature. It will not change, however the reaction attains equilibrium 10 times faster hence

$K_{\text{(new) }}+K_{\text{(previous} }}=4\times 10^{-4}$