Chemistry - Thermochemistry Question with Solution | TestHub

The enthalpy changes for the following processes are listed below: $\begin{array}{ll}{\mathrm{Cl}}_2(\mathrm{g})=2\mathrm{Cl}(\mathrm{g}),& 242.3\mathrm{kJ}{\mathrm{mol}}^{-1}\\ {\mathrm{I}}_2(\mathrm{g})=2\mathrm{I}(\mathrm{g}),& 151.0\mathrm{kJ}{\mathrm{mol}}^{-1}\\ \mathrm{ICl}(\mathrm{g})=\mathrm{I}(\mathrm{g})+\mathrm{Cl}(\mathrm{g}),& 211.3\mathrm{kJ}{\mathrm{mol}}^{-1}\\ {\mathrm{I}}_2(\mathrm{s})={\mathrm{I}}_2(\mathrm{g}),& 62.76\mathrm{kJ}{\mathrm{mol}}^{-1}\end{array}$ Given that the standard states for iodine and chlorine are ${\mathrm{I}}_2(\mathrm{s})$ and ${\mathrm{Cl}}_2(\mathrm{g})$, the standard enthalpy of formation for $\mathrm{ICl}(\mathrm{g})$ is