(Solved): 9) Calculate the lattice energy of magnesium sulfide from the data given below. \[ \begin{array}{l} ...

9) Calculate the lattice energy of magnesium sulfide from the data given below. \[ \begin{array}{l} \mathrm{Mg}(s) \rightarrow \mathrm{Mg}(g) \Delta H^{\circ}=148 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Mg}(g) \rightarrow \mathrm{Mg}^{2+}(g)+2 \mathrm{e}^{-} \Delta H^{\circ}=2186 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{S}(s) \rightarrow 8 \mathrm{~S}(g) \Delta H^{\circ}=2232 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{S}(g)+2 \mathrm{e}^{-} \rightarrow \mathrm{S}^{2-}(g) \Delta H^{\circ}=450 \mathrm{~kJ} / \mathrm{mol} \\ 8 \mathrm{Mg}(s)+\mathrm{S}_{8}(s) \rightarrow 8 \mathrm{MgS}(s) \Delta H^{\circ}=-2744 \mathrm{~kJ} / \mathrm{mol} \end{array} \] \[ \mathrm{Mg}^{2+}(g)+\mathrm{S}^{2-}(g) \rightarrow \underline{\mathrm{MgS}}(s) \Delta \underline{H}^{\circ \text { latticc }}=? \] A) \( 2720 . \mathrm{kJ} / \mathrm{mol} \) B) \( 3406 \mathrm{~kJ} / \mathrm{mol} \) C) \( -3406 \mathrm{~kJ} / \mathrm{mol} \) D) \( -2720 . \mathrm{kJ} / \mathrm{mol} \)