Thermodynamics

Consider the reaction

\(2 \mathrm{H}_2 \mathrm{~S}(\mathrm{~g})+3 \mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(\mathrm{l})+2 \mathrm{SO}_2(\mathrm{~g})\)

The magnitude of enthalpy change for the reaction in $\mathrm{kJ} \mathrm{mol}^{-1}$ is $\_\_\_\_$ . (Nearest integer)

$$ \begin{aligned} Given:\,\,& \Delta_{\mathrm{f}} \mathrm{H}^{\ominus}\left(\mathrm{H}_2 \mathrm{~S}\right)=-20.1 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\ominus}\left(\mathrm{H}_2 \mathrm{O}\right)=-286.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\ominus}\left(\mathrm{SO}_2\right)=-297.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned} $$