Consider the following heat changes in the oxidation of magnesium and iron.

Reaction involved:

(i) \(\mathrm{Mg}+\frac{1}{2} \mathrm{O}_{2}=\mathrm{MgO} \quad \Delta H=-602.06 \mathrm{~kJ} / \mathrm{mol}\)

(ii) \(2 \mathrm{Fe}+\frac{3}{2} \mathrm{O}_{2}=\mathrm{Fe}_{2} \mathrm{O}_{3} \quad \Delta H=-810.14 \mathrm{~kJ} / \mathrm{mol}\)

Calculate the heat produced in the reaction.

\[ 3 \mathrm{Mg}+\mathrm{Fe}_{2} \mathrm{O}_{3}=3 \mathrm{MgO}+2 \mathrm{Fe} \]