The standard electrode potential of a half-cell containing F2 g and F- ion can be calculated using the Nernst equation. The Nernst equation relates the reduction potential of a half-cell to the standard reduction potential, temperature, and concentrations of the species involved in the redox reaction. The equation is as follows:E = E - RT/nF * ln Q where:E = the electrode potential of the half-cellE = the standard reduction potential of the half-cellR = the gas constant 8.314 J/molK T = the temperature in Kelvin 25C = 298.15 K n = the number of electrons transferred in the redox reaction for F2/F-, n = 2 F = the Faraday constant 96,485 C/mol Q = the reaction quotient, which is the ratio of the concentrations of the products to the reactants raised to their stoichiometric coefficientsFor the half-cell containing F2 g and F- ion, the redox reaction is:F2 g + 2e- -> 2F- aq The standard reduction potential for F2 g is 2.87 V, and the standard reduction potential for F- ion is -2.87 V. Since we are considering the reduction of F2 g to F- ion, we will use the standard reduction potential of F2 g , which is 2.87 V. In this case, we are not given the concentrations of F2 g and F- ion, so we cannot calculate the exact electrode potential using the Nernst equation. However, we can still determine the standard electrode potential, which is the potential when all species are at their standard states 1 M for F- ion and 1 atm for F2 g .Under standard conditions, the reaction quotient Q is equal to 1, and the natural logarithm of 1 is 0. Therefore, the Nernst equation simplifies to:E = ESo, the standard electrode potential of the half-cell containing F2 g and F- ion at 25C is equal to the standard reduction potential of F2 g , which is 2.87 V.