Question

n mole of $PCl _{3}$ and $n$ mole of $Cl _{2}$ are allowed to react at constant temperature $T$ to have a total equilibrium pressure $P_{1}$ as :

$PCl _{3}( g )+ Cl _{2}( g ) \rightleftharpoons PCl _{5}( g )$

If $y$ mole of $PCl _{5}$ are formed at equilibrium, find $K _{p}$ for the given reaction.

(A) $\frac{(2 n-y) y}{(n-y)^{2} \cdot P}$

(B) $\frac{y}{(n-y)^{2}(2 n-y) P}$

(C) $\frac{(n-y)^{2} \cdot P}{(2 n-y) y}$

(D) $\frac{(n-y)^{2}(2 n-y) P}{y}$

Answer 1

If $y$ mole of $PCl _{5}$ are formed at equilibrium, then $K _{p}$ for the given reaction will be $\frac{(2 n-y) y}{(n-y)^{2} \cdot P}$.

So, The correct option of this question is (A)