$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}\phantom{\rule{0ex}{0ex}}\mathbf{\Delta G}{\mathbf{\xb0}}_{\mathbf{rxn}}\mathbf{=}\mathbf{-}\mathbf{(}\mathbf{8}\mathbf{.}\mathbf{314}\mathbf{}\frac{\mathbf{J}}{\mathbf{mol}\mathbf{\xb7}\mathbf{K}}\mathbf{)}\mathbf{(}\mathbf{298}\mathbf{}\mathbf{K}\mathbf{)}\mathbf{}\mathbf{ln}\mathbf{}\mathbf{(}\mathbf{81}\mathbf{.}\mathbf{9}\mathbf{)}$

Calculate G_{rxn} at 298 K for the following reaction: I_{2}(s) + Cl_{2}(g) ⇌ 2 (g), K_{p} = 81.9

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