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Hess' Law

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Question

Calculate the enthalpy of the reaction:
$S n O_{2} (s) + 2 H_{2} (g) ⟶ S n (s) + 2 H_{2} O (l)$
given that, enthalpies of formation of $S n O_{2} (s)$ and $H_{2} O (l)$ are $- 580.7 k J$ and $- 285.8 k J$ respectively.

A

- 9.1 k J

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B

+ 9.1 k J

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C

- 8.1 k J

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D

+ 8.1 k J

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Solution

The correct option is B $+ 9.1 k J$
Enthalpy of reaction = 2 $\times$ enthalpy of fromation of water - enthalpy of formation of $S N O_{2}$
Enthalpy of reaction = $2 * (- 285.8) - (- 580.7) = 9.1 k J$

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