Chemistry - Thermochemistry Question with Solution | TestHub

Given Reaction Energy Change $\begin{array}{ll}& \text{ (in kJ) }\\ \mathrm{Li}(\mathrm{s})\to \mathrm{Li}(\mathrm{g})& 161\\ \mathrm{Li}(\mathrm{g})\to {\mathrm{Li}}^{+}(\mathrm{g})& 520\\ \frac{1}{2}{\mathrm{F}}_2(\mathrm{g})\to \mathrm{F}(\mathrm{g})& 77\\ \mathrm{F}(\mathrm{g})+{\mathrm{e}}^{-}\to {\mathrm{F}}^{-}(\mathrm{g})& \begin{array}{l}\text{ (Electron gain }\\ \text{ enthalpy) }\end{array}\\ {\mathrm{Li}}^{+}(\mathrm{g})+{\mathrm{F}}^{-}(\mathrm{g})\to \mathrm{LiF}(\mathrm{s})& -1047\\ \mathrm{Li}(\mathrm{s})+\frac{1}{2}{\mathrm{F}}_2(\mathrm{g})\to \mathrm{LiF}(\mathrm{s})& -617\end{array}$ Based on data provided, the value of electron gain enthalpy of fluorine would be :