To calculate the Gibbs free energy change G of a spontaneous electrochemical reaction, we can use the following equation:G = -nFEwhere:- n is the number of moles of electrons transferred in the reaction- F is the Faraday constant 96,485 C/mol - E is the cell potential 1.10 V in this case For the reaction between zinc and copper, the balanced redox reaction is:Zn s + Cu^2+ aq Zn^2+ aq + Cu s In this reaction, 2 moles of electrons are transferred n = 2 as zinc loses 2 electrons and copper gains 2 electrons.Now we can plug the values into the equation:G = - 2 mol 96,485 C/mol 1.10 V G = -212,667 J/molThe Gibbs free energy change for this spontaneous electrochemical reaction is -212,667 J/mol.