To calculate the standard Gibbs free energy change G for the given electrochemical reaction, we first need to determine the overall cell potential E for the reaction. The overall cell potential can be found by subtracting the standard reduction potential of the half-reaction being oxidized from the standard reduction potential of the half-reaction being reduced. In this case, Cu s is being oxidized to Cu aq , and Ag aq is being reduced to Ag s .E cell = E reduction - E oxidation Since the given half-reactions are:Cu aq + 2e Cu s E = +0.34 V reduction Ag aq + e Ag s E = +0.80 V reduction We need to reverse the Cu aq + 2e Cu s half-reaction to represent the oxidation of Cu s to Cu aq :Cu s Cu aq + 2e E = -0.34 V oxidation Now we can calculate the overall cell potential:E cell = E reduction - E oxidation E cell = +0.80 V - -0.34 V E cell = +1.14 VNow that we have the overall cell potential, we can calculate the standard Gibbs free energy change G using the following equation:G = -nFEwhere n is the number of moles of electrons transferred in the reaction, F is the Faraday constant 96,485 C/mol , and E is the overall cell potential.In this reaction, 2 moles of electrons are transferred from Cu to 2Ag :G = - 2 mol 96,485 C/mol +1.14 V G = -219,663.8 J/molSince the standard Gibbs free energy change is typically expressed in kJ/mol, we can convert it:G = -219.66 kJ/molSo, the standard Gibbs free energy change G for the given electrochemical reaction is -219.66 kJ/mol.