The enthalpy changes for the following processes are listed   below : 
$$\begin{gathered} {\mathrm{Cl}}_2\left(\mathrm{g}\right)\to 2\mathrm{Cl}\left(\mathrm{g}\right) 242.3\mathrm{kJ}{\mathrm{mol}}^{-1} \\ {\mathrm{I}}_2\left(\mathrm{g}\right)\to 2\mathrm{I}\left(\mathrm{g}\right) 151.0\mathrm{kJ}{\mathrm{mol}}^{-1} \\ \mathrm{ICl}\left(\mathrm{g}\right)\to \mathrm{I}\left(\mathrm{g}\right)+\mathrm{Cl}\left(\mathrm{g}\right) 211.3\mathrm{kJ}{\mathrm{mol}}^{-1} \\ {\mathbf{I}}_2\left(\mathrm{s}\right)\to {\mathrm{I}}_2\left(\mathrm{g}\right) 62.76\mathrm{kJ}{\mathrm{mol}}^{-1} \end{gathered}$$
Given that the standard states for iodine and chlorine are  ${\mathrm{I}}_2\left(\mathrm{s}\right)\text{ and }{\mathrm{Cl}}_2\left(\mathrm{g}\right)$the standard enthalpy of formation for ICI(g)  is :