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Equipartition Theorem

The heat of r...

Question

The heat of reaction for, $C_{10} H_{8 (s)} + 12 O_{2 (g)} \to 10 C O_{2 (g)} + 4 H_{2} O_{(1)}$ at constant volume is $- 1228.2 k c a l$ at $25^{o} C$ . Calculate the heat of reaction at constant pressure at $25^{o} C .$

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Solution

Heat of reaction at constant pressure is represented by $Δ H$

Heat of reaction at constant volume is represented by $Δ U$

Given: $Δ U = - 1228.2$ kcal

Since $Δ H = Δ U + Δ n R T$

In the given reaction $Δ n = 10 - 12 = - 2$
$R = 2$ cal/mol K

$Δ H = - 1228.2 + (- 2 / 1000) (2 \times 298) = - 1229.4$ kcal

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