Question

Given the following:

2 Fe_{(s)} + 3/2 O_{2(g)} → Fe_{2}O_{3(s)} ΔH^{o}_{rxn} = -824.2 kJ/mol

3 Fe_{(s)} + 2 O_{2(g)} → Fe_{3}O_{4(s)} ΔH^{o}_{rxn} = -1118.4 kJ/mol

Calculate the ΔH^{o}_{rxn} for the following equation:

3 Fe_{2}O_{3(s)} → 2 Fe_{3}O_{4(s)} + 1/2 O_{2(g)}

Your answer should be to one place past the decimal point.

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