question_answer

The enthalpy changes for the following processes are listed below        \[\text{C}{{\text{l}}_{\text{2}}}\text{(g)}\to \text{2Cl(g),242}\text{.3 kJ mo}{{\text{l}}^{\text{-1}}}\] \[{{\text{I}}_{\text{2}}}\text{(g)}\to \text{2I(g),151}\text{.0 kJ mo}{{\text{l}}^{\text{-1}}}\] \[\text{ICl(g)}\to \text{I(g)+Cl(g),211}\text{.3 kJ mo}{{\text{l}}^{\text{-1}}}\] \[{{\text{I}}_{\text{2}}}\text{(g)}\to {{\text{I}}_{\text{2}}}\text{(g),62}\text{.76 kJ mo}{{\text{l}}^{\text{-1}}}\] Given that the standard states for iodine and chlorine are\[{{I}_{2}}(s)\] and \[C{{l}_{2}}(g),\] the standard enthalpy for the formation of \[ICl(g)\] is

A) \[-\text{14}.\text{6 kJ mo}{{\text{l}}^{\text{-1}}}\]      

B) \[-\text{16}.\text{8 kJ mo}{{\text{l}}^{\text{-1}}}\]

C) \[+\text{16}.\text{8 kJ mo}{{\text{l}}^{-}}^{\text{1}}\]    

D) \[+\text{244}.\text{8 kJ mo}{{\text{l}}^{\text{-1}}}\]