The equilibrium constant for the reaction N_{ | vedclass

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(A) catalyst provides an alternative reaction pathway with a lower activation energy, which increases the rate of both the forward and backward reacti

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$4 	imes 10^{-4}$

Vedclass · Answer

(A) catalyst provides an alternative reaction pathway with a lower activation energy, which increases the rate of both the forward and backward reactions equally.Since the rate of both reactions increases by the same factor, the equilibrium position remains unchanged.The equilibrium constant $(K_{eq})$ is a function of temperature only for a given reaction.Since the temperature remains constant at $2000 \ K$, the equilibrium constant remains $4 	imes 10^{-4}$.

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

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