To calculate the Gibbs free energy change G for the electrochemical reaction, we first need to determine the standard cell potential Ecell for the reaction. This can be done using the standard reduction potentials given:Ecell = E cathode - E anode In this reaction, Cu2+ is reduced to Cu, so it is the cathode, and Zn is oxidized to Zn2+, so it is the anode.Ecell = E Cu2+|Cu - E Zn2+|Zn = +0.34 V - -0.76 V = +1.10 VNow that we have the standard cell potential, we can calculate the Gibbs free energy change using the following equation:G = -nFEcellWhere n is the number of moles of electrons transferred in the reaction in this case, 2 moles of electrons, as both Cu2+ and Zn2+ have a charge of +2 , F is the Faraday constant 96,485 C/mol , and Ecell is the standard cell potential.G = -2 mol 96,485 C/mol 1.10 V = -212,667 J/molSince the value is usually expressed in kJ/mol, we can convert it:G = -212,667 J/mol 1 kJ/1000 J = -212.67 kJ/molSo, the Gibbs free energy change for the given electrochemical reaction at 25C is -212.67 kJ/mol.