The difference between heats of reaction at constant pressure and constant volume of the following reaction would be
$2 C_{6} H_{6} (l) + 15 O_{2} (g) ⟶ 12 C O_{2} (g) + 6 H_{2} O (l)$ at 25°C in kJ mol⁻¹ is

Question

The difference between heats of reaction at constant pressure and constant volume of the following reaction would be

$2 C_{6} H_{6} (l) + 15 O_{2} (g) ⟶ 12 C O_{2} (g) + 6 H_{2} O (l)$ at 25°C in kJ mol⁻¹ is

TestHub · Accepted Answer

Δ H = Δ U + Δ n g ​ RT ⇒ Δ H − Δ U = Δ n g ​ RT . = 1000 − 3 × 8.314 × 298 ​ = − 7.4327 k J m o l − 1

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