Initially $0.8 m o l e$ of $P C l_{5}$ and $0.2 m o l e$ of $P C l_{3}$ are mixed in one litre vessel. At equilibrium $0.4 m o l e$ of $P C l_{3}$ is present .
The value of $K_{c}$ for the reaction $P C l_{5 (g)} ⟺ P C l_{3 (g)} + C l_{2} (g)$

0.13 m o l L^{- 1}

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0.05 m o l L^{- 1}

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0.065 m o l L^{- 1}

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0.1 m o l L^{- 1}

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Solution

The correct option is A $0.13 m o l L^{- 1}$
$V o l u m e = k$
$P C l_{5 (g)} ⇌ P C l_{3} (g) + C l_{2} (g)$
$\begin{matrix} t = 0 t = t_{\infty} \end{matrix} ∣ ∣ ∣ \begin{matrix} 0.8 & 0.2 0.8 - x & 0.2 + x \end{matrix}$
Given,
$0.2 + x = 0.4$
$x = 0.2$
$K_{c} = \frac{[P C l_{3}] [C l_{2}]}{P C l_{5}}$
$= \frac{[0.4] [0.2]}{0.6}$
$= 0.13 m o l / L$

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