Use the given standard enthalpies of formation (in $\mathrm{kJ} / \mathrm{mol}$ ) to determine the enthalpy of reaction of the following reaction :
$$
\begin{gathered}
\mathrm{NH}_{3}(g)+3 \mathrm{~F}_{2}(g) \longrightarrow \mathrm{NF}_{3}(g)+3 \mathrm{HF}(g) \\
\Delta H_{f}^{\circ}\left(\mathrm{NH}_{3}, g\right)=-46.2 ; \quad \Delta H_{f}^{\circ}\left(\mathrm{NF}_{3}, g\right)=-113.0 ; \quad \Delta H_{f}^{\circ}(\mathrm{HF}, g)=-269.0
\end{gathered}
$$
1.T/mnl
(h) $-8738 \mathrm{~kJ} / \mathrm{mol}$
(c) $-697.2 \mathrm{~kJ} / \mathrm{mol}$
(d) $-890.4 \mathrm{~kJ} / \mathrm{mol}$