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Equilibrium Constant and Standard Free Energy Change

The reaction ...

Question

The reaction
$S O {C l}_{2} + H_{2} O ⟶ {S O}_{2} + 2 H C l$
is endothermic by $49.4 k J$ and exoergonic by $50.8 k J$ . What is the factor that makes the reaction to be spontaneous? Calculate the entropy change at $298 K$ .

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Solution

$Δ S^{o} = 0.3362 k J K^{- 1}$
Exoergonic means $Δ G^{o} = - v e$
$Δ G^{o} = - 50.8 k J$
$Δ H^{o} = 49.4 k J$
Substituting values in $Δ S^{o} = \frac{Δ H^{o} - Δ G^{o}}{T}$
$Δ S^{o} = 0.3362 k J K^{- 1}$

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