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Gibbs Free Energy & Spontaneity

Find the magn...

Question

Find the magnitude of enthalpy of formation of $H C l$ (in $k j m o l^{- 1}$ ) if the bond dissociation enthalpy of $H_{2}$ , $C l_{2}$ and $H C l$ are 434, 242 and 431 kj $m o l^{- 1}$ respectively.

A

105

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B

39

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C

93

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D

99

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Solution

The correct option is C $93$
$H_{2} + C l_{2} \to 2 H C l$

$Δ H = 434 + 242 - 2 (431) = - 186$

$∴ Δ H_{f} = \frac{Δ H}{2} = - 93$

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