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The equilibrium constant for the reaction
$N_{2} (g) + O_{2} (g) ⇌ 2 NO (g)$ is $4 \times 10^{- 4}$ at 200 K. In the presence of a catalyst the equilibrium is attained 10 times faster. Therefore the equilibrium constant in presence of the catalyst at 200 K is

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$4 \times 10^{- 3}$

$4 \times 10^{- 4}$

$4 \times 10^{- 5}$

None

answer is B.

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Detailed Solution

Equilibrium constant of a reaction remains unchanged when the same reaction is carried out in the presence of a catalyst because A catalyst speeds up both the forward and back reactions by exactly the same amount.

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