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When the molar concentrations of $S O_{2}, O_{2} a n d 2 S O_{3}$ at equilibrium at certain temperatures are 0.5, 0.25 & 0.25M respectively, $K_{c}$ for $2 S O_{3} ⇌ 2 S O_{2} + O_{2}$ is

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$1 l i t^{- 2} m o l^{- 2}$

$1 m o l l i t^{- 1}$

$1 m o l^{2} l i t^{- 2}$

$1 l i t - m o l^{- 1}$

answer is C.

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Detailed Solution

Given: It is given to find $K_{c}$ for reaction:

$2 S O_{3} ⇌ 2 S O_{2} + O_{2}$

At equilibrium concentrations are $[S O_{3}] = 0.25 M, [S O_{2}] = 0.5 M, [O_{2}] = 0.25 M$

Formula used= $K_{c} = [O_{2}] [S O_{2}]^{2} / [S O_{3}]^{2}$

Explanation: $K_{c} = [0.25] [0.5]^{2} / [0.25]^{2} = M^{3} / M^{2} = 1 M = 1 m o l l i t^{- 1}$

Hence, the correct option C is i.e., $1 m o l l i t^{- 1}$ .

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