To calculate the standard free energy change G for the redox reaction, we first need to determine the standard cell potential Ecell for the reaction. We can do this using the given standard reduction potentials E for the half-reactions:E Fe3+|Fe2+ = +0.77 VE Cl2|Cl- = +1.36 VSince Fe2+ is being oxidized to Fe3+ and Cl2 is being reduced to Cl-, the overall cell potential is:Ecell = E reduction - E oxidation Ecell = E Cl2|Cl- - E Fe3+|Fe2+ Ecell = +1.36 V - +0.77 V Ecell = +0.59 VNow that we have the standard cell potential, we can calculate the standard free energy change G using the following equation:G = -nFEcellwhere n is the number of moles of electrons transferred in the reaction, F is Faraday's constant 96,485 C/mol , and Ecell is the standard cell potential.In this reaction, 2 moles of electrons are transferred from 2Fe2+ to 2Fe3+ , so n = 2. Therefore:G = - 2 mol 96,485 C/mol +0.59 V G = -113,851.9 J/molSince the standard free energy change is typically expressed in kJ/mol, we can convert it:G = -113.85 kJ/molSo, the standard free energy change G for the given redox reaction at 298 K is -113.85 kJ/mol.