To calculate the standard free energy change G for the redox reaction, we first need to determine the standard cell potential E for the reaction. The equation to relate G and E is:G = -nFEwhere n is the number of moles of electrons transferred in the reaction, F is the Faraday constant 96,485 C/mol , and E is the standard cell potential.First, we need to find the standard reduction potentials for the half-reactions:Fe^3+ aq + e^- Fe^2+ aq E = +0.77 VCl2 g + 2e^- 2 Cl^- aq E = +1.36 VNow, we need to reverse the first half-reaction to make it an oxidation reaction:Fe^2+ aq Fe^3+ aq + e^- E = -0.77 VNow, we can add the two half-reactions to get the overall redox reaction:2 Fe^2+ aq + Cl2 g 2 Fe^3+ aq + 2 Cl^- aq The overall standard cell potential E is the sum of the standard potentials of the two half-reactions:E = -0.77 V + +1.36 V = +0.59 VNow, we can calculate the standard free energy change G :G = -nFEIn this reaction, n = 2 moles of electrons are transferred. Therefore,G = - 2 mol 96,485 C/mol 0.59 V = -113,932 J/molWe can convert this to kJ/mol:G = -113.932 kJ/molSo, the standard free energy change for the redox reaction of 2 Fe^2+ aq + Cl2 g 2 Fe^3+ aq + 2 Cl^- aq at 298 K is -113.932 kJ/mol.