Two reactions are given below: 2 Fe_( s ) +3/2 O_2( g ) → Fe_2 O_3( s ), Δ H^°=-822 kJ / mol; C_( s ) +1/2 O_2( g ) → CO_( g ), Δ H^°=-110 kJ / mol…

Two reactions are given below: $$\begin{aligned} & 2 \mathrm{Fe}_{(\mathrm{s})}+\frac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{Fe}_2 \mathrm{O}_{3(\mathrm{~s})}, \Delta \mathrm{H}^{\circ}=-822 \mathrm{~kJ} / \mathrm{mol} \\ & \mathrm{C}_{(\mathrm{s})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{(\mathrm{g})}, \Delta \mathrm{H}^{\circ}=-110 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Then enthalpy change for following reaction $\displaystyle 3 \mathrm{C}_{(\mathrm{s})}+\mathrm{Fe}_2 \mathrm{O}_{3(\mathrm{~s})} \rightarrow 2 \mathrm{Fe}_{(\mathrm{s})}+3 \mathrm{CO}_{(\mathrm{g})}$ is $\displaystyle \_\_\_\_$ $\displaystyle \mathrm{kJ} / \mathrm{mol}$.