The enthalpy changes for the following processes are listed below \[\] $Cl_2(g) = 2Cl(g),\: \: \: \: \: 242.3\: kJ/mol$ \[\] $I_2(g) = 2I(g), \: \: \: \: \: 151\: kJ/mol$ \[\] $ ICl(g) = I(g) + Cl(g),\: \: \: 211.3 \: kJ/mol$ \[\] $ I_2(s) = I_2(g),\: \: \: \: 62.76\: kJ/mol$ \[\] Given that the standard states for iodine and chlorine are $I_2(g)\: and \: Cl_2(g)$, the standard enthalpy of formation of $ICl(g)$ is

Question

$\begin {array} {1 1} (A)\;-14.6\: kJ/mol & \quad (B)\;-244.8\: kJ/mol \\ (C)\;16.8\: kJ/mol & \quad (D)\;244.8\: kJ/mol \end {array}$