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When the molar concentrations of ${SO}_{2}, O_{2}$ and ${SO}_{3}$ at equilibrium at certain temperature are 0.5, 0.25 & 0.25M respectively, $K_{c}$ for $2 {SO}_{3} ⇌ 2 {SO}_{2} + O_{2}$ is

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1mol - lit^-1

1lit² - mol^-1

0.5lit mol^-1

0.25mol² - lit^-2

answer is C.

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Detailed Solution

$K_{c} = \frac{{({SO}_{2})}^{2} (O_{2})}{({SO}_{3})} = \frac{{(0.5)}^{2} (0.25)}{{(0.25)}^{2}} = 1 mole - {lit}^{- 1} .$

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