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Characteristics of Equilibrium Constant

PCl5, PCl3 an...

Question

$P C l_{5}, P C l_{3} a n d C l_{2}$ are at equilibrium at $500$ K with concentration $2.1$ M $P C l_{3}, 2.1 M C l_{2}$ and $1.9 M P C l_{5}$ . The equilibrium constant for the given reaction is:
$P C l_{5 (g)} ⇌ P C l_{3 (g)} + C l_{2 (g)}$

2.32

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1.79

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4.2

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3.8

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Solution

The correct option is A $2.32$
$P C l_{5} ⇌ P C l_{3} + C l_{2}$
$K_{c} = \frac{[P C l_{3}] [C l_{2}]}{[P C l_{5}]}$
$K_{c} = \frac{2.1 \times 2.1}{1.9}$
$K_{c} = \frac{4.41}{1.9}$
$∴$ the equilibrium constant of the above reaction $K_{c} = 2.321$

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