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Hydrogenation of Alkynes

If the bond e...

Question

If the bond energies of $H - H$ , $B r - B r$ , and $H - B r$ are $433, 192$ and $364 {kJ mol}^{- 1}$ respectively, the $Δ H^{o}$ for the reaction $H_{2} (g) + B r_{2} (g) \to 2 H B r (g)$ is:

A

- 261 kJ

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B

+ 103 kJ

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C

+ 261 kJ

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D

- 103 kJ

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Solution

The correct option is D $- 103 kJ$
We know that,
$H_{2} + B r_{2} \to 2 H B r$
$H - H 433 + B r - B r 192 \to 2 H - B r 2 \times 364 = 728$
Net energy released $= 728 - 433 - 192 = 103 kJ$
Since, energy is released, $Δ H^{o} = - 103 kJ$ .

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