To calculate the change in Gibbs free energy G for the electrochemical reaction, we first need to determine the overall cell potential Ecell for the redox reaction. The cell potential is the difference between the reduction potentials of the two half-reactions.In this case, the Cu2+ half-reaction is the reduction half-reaction, and the Fe2+ half-reaction needs to be reversed to become an oxidation half-reaction:Cu2+ aq + 2e- Cu s E = +0.34 V reduction Fe s Fe2+ aq + 2e- E = +0.44 V oxidation, reversed sign Now, we can calculate the overall cell potential Ecell :Ecell = E reduction + E oxidation Ecell = +0.34 V + +0.44 V Ecell = +0.78 VNext, we can use the Nernst equation to calculate the change in Gibbs free energy G :G = -nFEcellwhere n is the number of moles of electrons transferred in this case, n = 2 , F is Faraday's constant 96,485 C/mol , and Ecell is the overall cell potential.G = - 2 mol 96,485 C/mol 0.78 V G = -150,356.2 J/molThe change in Gibbs free energy for the electrochemical reaction is -150,356.2 J/mol.