To calculate the Gibbs free energy change G for the reaction, we first need to determine the overall cell potential E for the redox reaction using the standard reduction potentials for each half-reaction.The half-reactions are:1. Oxidation of Zinc: Zn s Zn aq + 2eStandard reduction potential E = -0.76 V2. Reduction of Copper ions: Cu aq + 2e Cu s Standard reduction potential E = +0.34 VSince the Zinc is being oxidized, we need to reverse the sign of its standard reduction potential. The overall cell potential E is the sum of the standard reduction potentials for the two half-reactions:E = E - E = +0.34 V - -0.76 V = +1.10 VNow, we can calculate the Gibbs free energy change G using the formula:G = -nFEwhere n is the number of moles of electrons transferred in this case, 2 moles of electrons , F is the Faraday constant approximately 96,485 C/mol , and E is the overall cell potential.G = -2 mol 96,485 C/mol 1.10 VG = -212,267 J/molThe Gibbs free energy change for the reaction of Zinc with Copper sulfate solution is -212,267 J/mol.