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Determine the enthalpy change for the reaction of 5.00 g of ${Fe}_{2} O_{3}$ with aluminium metal according to the equation :
${Fe}_{2} O_{3} (s) + 2 Al (s) ⟶ {Al}_{2} O_{3} (s) + 2 Fe (l)$
Substance $Δ H_{f}^{\circ} kJ / mol$
${Fe}_{2} O_{3} (s)$ -825.5
${Al}_{2} O_{3} (s)$ -1675.7
$Fe (l)$ 12.4

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- 26.6 kJ

- 52.4 kJ

-28.2 kJ

- 77.9 kJ

answer is A.

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Detailed Solution

$\begin{array}{l} Δ H = \frac{5}{56 \times 2 + 3 \times 16} [- 1675.7 + 12.4 - (- 825 \cdot 5)] \\ = \frac{5}{160} [- 1675.7 + 12.4 + 825.5) \\ = - 26.1825 KJ \end{array}$

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