To calculate the standard electrode potential for the given cell, we can use the Nernst equation:E_cell = E_cell - RT/nF * ln Q where E_cell is the cell potential, E_cell is the standard cell potential, R is the gas constant 8.314 J/molK , T is the temperature in Kelvin assume 298 K , n is the number of electrons transferred, F is the Faraday constant 96485 C/mol , and Q is the reaction quotient.First, we need to determine the balanced redox reaction and the standard cell potential E_cell . The half-reactions are:Mg -> Mg + 2e oxidation 2Ag + 2e -> 2Ag reduction The balanced redox reaction is:Mg + 2Ag -> Mg + 2AgNow, we can calculate the standard cell potential E_cell :E_cell = E Ag/Ag - E Mg/Mg = 0.80 V - -2.37 V = 3.17 VNext, we need to determine the reaction quotient Q :Q = [Mg]/[Ag]^2 = 0.10 M / 1.0 M ^2 = 0.10Now we can plug the values into the Nernst equation:E_cell = 3.17 V - 8.314 J/molK * 298 K / 2 * 96485 C/mol * ln 0.10 E_cell = 3.17 V - 0.0257 V * ln 0.10 E_cell = 3.17 V - -0.0591 V E_cell = 3.2291 VThe standard electrode potential for the given cell is approximately 3.23 V.