Answer:
Free energy change of the reaction is +98.83 kJ/mol.
Explanation:
The dissociation reaction of mercury(I) aqueous solution is as follows.
[tex]Hg_{2}Cl_{2}(s)\rightarrow Hg_{2}^{2+}(aq)+2Cl^{-}(aq)[/tex]
The standard free energy of the reaction is as follows.
[tex]\Delta G_{rxn}^{o}=m\Delta G^{o}(products)-n\Delta G^{o}_{reactants}[/tex]
[tex]=[(1\times \Delta G^{o}_{f(Hg_{2}^{2+})})+(2\times \Delta G^{o}_{f(Cl^{-})})-(1\times \Delta G^{o}_{f(Hg_{2}Cl_{2})})][/tex]
[tex]=[(1\times 153.5+2\times -131.25)-(1\times -210.78)]kJ=+101.78kJ[/tex]
[tex]Gas\,constant"R"=8.314\times 10^{-3}kJK^{-1}mol^{-1}[/tex]
[tex]Temperature=25^{o}c=25+273=298K[/tex]
[tex]Free\,energy\,change\,of\,the\,reaction=\Delta G=\Delta G^{o}+RT\,lnQ[/tex]
[tex]\Delta G=\Delta G^{o}+RT\,ln([Hg_{2}^{2+}][Cl^{-}]^{2})[/tex]
[tex]=(101.78kJ)+8.314\times 10^{-3}kJK^{-1}mol^{-1}\times298K ln((0.926)(0.573)^{2})[/tex]
[tex]=(101.78kJ)+(-2.95kJ)=+98.83kJ/mol[/tex]
Therefore, Free energy change of the reaction is +98.83 kJ/mol.
