(Solved): 1. Using the enthalpies for the following processes, calculate the lattice enthalpy for \( \mathrm ...

1. Using the enthalpies for the following processes, calculate the lattice enthalpy for \( \mathrm{NaCl} \). \[ \begin{array}{l} \mathrm{Na}^{+}(g)+\mathrm{Cl}^{-}(g) \longrightarrow \mathrm{NaCl}(s) \quad \Delta H_{\text {xtal }}=? \quad \text { Lattice enthalpy } \\ \mathrm{Na}(\mathrm{s}) \longrightarrow \mathrm{Na}(\mathrm{g}) \longrightarrow \Delta \mathrm{H}_{\text {sub }}=109 \mathrm{~kJ} / \mathrm{mol} \quad \text { Sublimation } \\ \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{Cl}(g) \quad \Delta H_{\mathrm{dis}}=239 \mathrm{~kJ} / \mathrm{mol} \text { Dissociation } \\ \mathrm{Na}(g) \longrightarrow \mathrm{Na}^{+}(g)+\mathrm{e}^{-} \quad \Delta H_{\text {ion }}=496 \mathrm{~kJ} / \mathrm{mol} \quad \text { Ionization } \\ \mathrm{Cl}^{-}(g) \longrightarrow \mathrm{Cl}(g)+\mathrm{e}^{-} \quad \Delta H_{\text {ea }}=349 \mathrm{~kJ} / \mathrm{mol} \quad \text { Electron affinity } \\ \mathrm{Ja}^{+}(s)+1 / 2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NaCl}(s) \quad \Delta H_{\mathrm{ea}}=-413 \mathrm{~kJ} / \mathrm{mol} \quad \text { Formation enthalpy } \\ \end{array} \]