Easy
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:
- A$4 \times 10^{-4}$
- B$4 \times 10^{-3}$
- C$4 \times 10^{-5}$
- D$2.5 \times 10^{-4}$
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View SolutionThe equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ 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 a catalyst at $2000 \ K$ is:
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