To calculate the standard Gibbs free energy change G for the electrochemical reaction, we first need to determine the standard cell potential E for the reaction. This can be found by subtracting the standard electrode potential of the reduction half-reaction from the standard electrode potential of the oxidation half-reaction.The given standard electrode potentials are:E Cu2+ aq + 2e- Cu s = 0.34 V reduction half-reaction E Zn2+ aq + 2e- Zn s = -0.76 V reduction half-reaction Since Zn is oxidized in the reaction, we need to reverse the Zn half-reaction to make it an oxidation half-reaction:E Zn s Zn2+ aq + 2e- = +0.76 V oxidation half-reaction Now we can calculate the standard cell potential E for the overall reaction:E cell = E reduction - E oxidation = 0.34 V - -0.76 V = 1.10 VNext, we can use the relationship between the standard cell potential and the standard Gibbs free energy change:G = -nFEwhere n is the number of moles of electrons transferred in the reaction in this case, 2 moles of electrons , F is Faraday's constant 96,485 C/mol , and E is the standard cell potential.G = - 2 mol 96,485 C/mol 1.10 V = -212,267 J/molSince the standard Gibbs free energy change is typically expressed in kJ/mol, we can convert the units:G = -212,267 J/mol * 1 kJ/1000 J = -212.27 kJ/molSo, the standard Gibbs free energy change G for the electrochemical reaction of zinc and copper ions is -212.27 kJ/mol.