To calculate the Gibbs free energy change G for the electrochemical reaction, we first need to determine the overall cell potential E_cell for the reaction. The cell potential can be calculated using the standard reduction potentials of the two half-reactions involved.The overall reaction can be written as:Zn s + 2H+ aq Zn2+ aq + H2 g The half-reactions are:1. Oxidation of Zn: Zn s Zn2+ aq + 2e- E = -0.76 V 2. Reduction of H+: 2H+ aq + 2e- H2 g E = 0 V Now, we can calculate the overall cell potential E_cell by subtracting the standard reduction potential of the oxidation half-reaction from the standard reduction potential of the reduction half-reaction:E_cell = E reduction - E oxidation E_cell = 0 V - -0.76 V E_cell = 0.76 VNow that we have the cell potential, we can calculate the Gibbs free energy change G using the following equation:G = -nFE_cellwhere n is the number of moles of electrons transferred in the reaction in this case, n = 2 , F is the Faraday constant approximately 96,485 C/mol , and E_cell is the cell potential.G = - 2 mol 96,485 C/mol 0.76 V G = -146,327.6 J/molSince we usually express Gibbs free energy change in kJ/mol, we can convert the value:G = -146.33 kJ/molSo, the Gibbs free energy change for the electrochemical reaction where zinc metal is oxidized by aqueous hydrogen ions to form aqueous zinc ions and hydrogen gas at 298 K is -146.33 kJ/mol.