To calculate the standard free energy change G for the redox reaction, we can use the Nernst equation:G = -n * F * Ewhere:G = standard free energy changen = number of moles of electrons transferred in the redox reactionF = Faraday's constant 96,485 C/mol E = standard cell potential difference in standard reduction potentials First, we need to determine the number of moles of electrons transferred n in the redox reaction. The balanced half-reactions are:Fe3+ aq + e- Fe2+ aq reduction half-reaction H2 g 2 H+ aq + 2 e- oxidation half-reaction Since there are 2 moles of Fe3+ reduced to Fe2+ in the overall reaction, the total number of moles of electrons transferred n is 2.Next, we need to calculate the standard cell potential E . Since the reaction is written as a reduction, we can use the given standard reduction potentials:E = E cathode - E anode E = E Fe3+/Fe2+ - E H+/H2 E = -0.771 V - 0.00 V E = -0.771 VNow, we can plug the values into the Nernst equation to calculate the standard free energy change G :G = -n * F * EG = -2 * 96,485 C/mol * -0.771 V G = 148,949.47 J/molSince the standard free energy change is typically expressed in kJ/mol, we can convert the value:G = 148,949.47 J/mol * 1 kJ / 1000 J G = 148.95 kJ/molTherefore, the standard free energy change for the given redox reaction under standard conditions is 148.95 kJ/mol.