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Enthalpy

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Question

Use the bond energies to estimate $Δ H$ for this reaction:
$H_{2} (g) + O_{2} (g) ⟶ H_{2} O_{2} (g)$
Bond Bond energy
$H - H$ $436 k J$ ${m o l}^{- 1}$
$O - O$
$142 k J$ ${m o l}^{- 1}$

$O = O$
$499 k J$ ${m o l}^{- 1}$

$H - O$
$460 k J$ ${m o l}^{- 1}$

A

- 127 k J

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B

- 209 k J

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C

- 484 k J

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D

- 841 k J

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Solution

The correct option is A $- 127 k J$
$Δ H = Σ b o n d e n e r g y o f r e a c t a n t - Σ b o n d e n e r g y o f p r o d u c t$
$δ H = (436 + 499) - (460 + 142 + 460)$
$Δ H = - 127 k J$

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