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. We can do this by finding the difference in the standard reduction potentials of the two half-reactions.The balanced half-reactions are:Fe3+ aq + e- Fe2+ aq E = -0.037 V reduction of Fe3+ I2 s + 2e- 2I- aq E = 0.535 V reduction of I2 Since the Fe3+ half-reaction is being reduced and the I2 half-reaction is being oxidized, we need to reverse the I2 half-reaction and change the sign of its standard reduction potential:2I- aq I2 s + 2e- E = -0.535 V oxidation of I- Now, we can add the two half-reactions and their standard potentials to find the overall cell potential E :2Fe3+ aq + 2I- aq 2Fe2+ aq + I2 s + 2e- + 2e-E = -0.037 V + -0.535 V = -0.572 VNext, we can use the Nernst equation to calculate the standard free energy change G :G = -nFEwhere n is the number of moles of electrons transferred in this case, 2 , F is the Faraday constant 96,485 C/mol , and E is the overall cell potential.G = - 2 96,485 C/mol -0.572 V G = 110,533 J/molSince the standard free energy change is usually expressed in kJ/mol, we can convert the value:G = 110.533 kJ/molSo, the standard free energy change G for the redox reaction at 298 K is 110.533 kJ/mol.