To calculate the standard free energy change G for the redox reaction, we first need to determine the overall cell potential E for the reaction. The cell potential is the difference between the standard reduction potentials of the two half-reactions.The given reaction can be divided into two half-reactions:1. Ag aq + e Ag s Reduction half-reaction 2. Cu s Cu aq + 2e Oxidation half-reaction The standard reduction potential E for the reduction half-reaction is given as +0.80 V, and the standard reduction potential for the oxidation half-reaction is given as +0.34 V. However, we need to reverse the oxidation half-reaction to find its standard oxidation potential:Cu aq + 2e Cu s The standard oxidation potential for the reversed reaction is -0.34 V.Now, we can calculate the overall cell potential E for the redox reaction:E = E reduction - E oxidation E = +0.80 V - -0.34 V E = +1.14 VNext, we can use the relationship between the standard free energy change G and the cell potential E to calculate G:G = -nFEwhere n is the number of moles of electrons transferred in the reaction, F is Faraday's constant 96,485 C/mol , and E is the cell potential.In this reaction, 2 moles of electrons are transferred from Cu to Ag . Therefore, n = 2.G = - 2 mol 96,485 C/mol 1.14 V G = -219,664.6 J/molSince the standard free energy change is typically expressed in kJ/mol, we can convert the value:G = -219.7 kJ/molSo, the standard free energy change G for the given redox reaction is -219.7 kJ/mol.