$N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)$ is a gaseous phase equilibrium reaction taking place in a $5$ litre flask at $1 a t m$ . For this :

K_{C} = K_{p}

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K_{C} = 25 K_{p}

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K_{p} = 25 K_{c}

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K_{C} = 5 K_{p}

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Solution

The correct option is B $K_{C} = 25 K_{p}$
We know,
$K_{p} = K_{c} (R T)^{Δ n_{g}}$
Here, $Δ n_{g} = 2 - 4 = - 2$
$K_{c} = K_{p} (R T)^{2}$
$= K_{p} (P V)^{2} = K_{p} (25) = 25 K_{p}$

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