Calculate the enthalpy change $(Δ H)$ in , $kJ {mol}^{- 1},$ of the following reaction
$2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 {CO}_{2} (g) + 2 H_{2} O (g)$
given average bond enthalpies of various bonds, i.e., $C - H, C \equiv C, O = O, C = O, O - H$ as $414, 814, 499,$ $724$ and $640 kJ {mol}^{- 1}$ respectively. Express magnitude only.

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answer is 2573.

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Detailed Solution

the enthalpy change $(Δ H)$ in , $kJ {mol}^{- 1},$ of the following reaction

$2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 {CO}_{2} (g) + 2 H_{2} O (g)$

$Δ_{r} H = 2 [814 + 2 \times 414] + 5 \times 499 - 8 \times 724 - 4 \times 640$

$= - 2573 kJ / mole$

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