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Q.

The heat of reaction for,
$C_{10} H_{8} (s) + 12 O_{2} (g) \to 10 {CO}_{2} (g) + 4 H_{2} O (l)$ , at constant volume is -122.2 k cal at 25°C. Calculate the heat of reaction at constant pressure at 25°C.

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answer is -1229.392.

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Detailed Solution

$\begin{array}{l} For C_{10} H_{8} (s) + 12 O_{2} (g) \to 10 {CO}_{2} (g) + 4 H_{2} O (1) \\ Given, Δ n = 10 - 12 = - 2; Δ U = - 1228.2 \times 10^{3} cal \\ T = 298 K; R = 2 cal \\ ∴ Δ H = Δ U + Δ n R T \\ = - 1228.2 \times 10^{3} + (- 2) \times 2 \times 298 = - 1229392 cal \\ = - 1229.392 kcal \end{array}$

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The heat of reaction for, C10H8(s)+12O2(g)→10CO2(g)+4H2O(l), at constant volume is -122.2 k cal at 25°C. Calculate the heat of reaction at constant pressure at 25°C.