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The enthalpy changes for the following processes are listed below :
\( \begin{array}{ll}\mathrm{Cl}_{2}(g) \rightarrow 2 \mathrm{Cl}(g), & 242.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_{2}(g) \rightarrow 2 \mathrm{I}(g), & 151.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{ICl}(g) \rightarrow \mathrm{I}(g)+\mathrm{Cl}(g), & 211.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_{2}(s) \rightarrow \mathrm{I}_{2}(g), & 62.76 \mathrm{~kJ} \mathrm{~mol}^{-1}\end{array} \)
Given that the standard states for iodine and chlorine are \( \mathrm{I}_{2}(s) \) and \( \mathrm{Cl}_{2}(g) \), the standard enthalpy of formation for \( \mathrm{ICl}(g) \)
- is:
(a) \( +16.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(b) \( +244.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(c) \( -14.6 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(d) \( -16.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
\( \mathrm{P} \)
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