To calculate the Gibbs free energy change G for the electrochemical reaction involving the oxidation of copper to copper II ions, we can use the following equation:G = -nFEwhere:- n is the number of moles of electrons transferred in the reaction for the oxidation of Cu to Cu2+, n = 2 - F is the Faraday's constant F = 96,485 C/mol - E is the cell potential E = 0.78 V Now, we can plug in the values and calculate G:G = - 2 mol 96,485 C/mol 0.78 V G = -150,676.2 J/molThe Gibbs free energy change for the electrochemical reaction involving the oxidation of copper to copper II ions in a solution of CuSO4 with a potential of 0.78 V at 25C is approximately -150.7 kJ/mol.