Answer:
The ΔG° for the dissolution of AgCl solid is 55.7 kJ/mol.
Explanation:
The Gibbs free energy of the reaction is given by :
[tex]\Delta G_{rxn}^o=\sum[\Delta G^o_{f}]_{products}-\sum[\Delta G^o_{f}]_{reactants}[/tex]
So for reaction :
[tex]AgCl(s)\rightarrow Ag^+(aq)+Cl^-(aq)[/tex]
Gibbs free energy of formation of silver ions = [tex]\Delta G^o_{f,Ag^+}=77.1 kJ/mol[/tex]
Gibbs free energy of formation of chloride ions = [tex]\Delta G^o_{f,Cl^-}=-131.2 kJ/mol[/tex]
Gibbs free energy of formation of silver chloride solid= [tex]\Delta G^o_{f,AgCl}=-109.8 kJ/mol[/tex]
The Gibbs free energy of the reaction of dissolution of AgCl :[tex]\Delta G_{rxn}^o[/tex] :
[tex]\Delta G_{rxn}^o=[77.1 kJ/mol+(-131.2 kJ/mol)]-[-109.8 kJ/mol][/tex]
[tex]=55.7 kJ/mol[/tex]
The ΔG° for the dissolution of AgCl solid is 55.7 kJ/mol.
