To calculate the polarization of the copper-silver galvanic cell, we first need to determine the standard cell potential E for the cell. The half-cell reactions for copper and silver are:Cu aq + 2e Cu s E Cu/Cu = +0.34 VAg aq + e Ag s E Ag/Ag = +0.80 VThe overall cell reaction is:Cu aq + 2Ag s Cu s + 2Ag aq The standard cell potential E for the cell is the difference between the standard reduction potentials of the two half-cells:E cell = E Ag/Ag - E Cu/Cu = 0.80 V - 0.34 V = 0.46 VNow, we can use the Nernst equation to calculate the actual cell potential E under the given conditions:E = E - RT/nF * ln Q where R is the gas constant 8.314 J/molK , T is the temperature in Kelvin 25C + 273.15 = 298.15 K , n is the number of electrons transferred in the reaction 2 for this cell , F is the Faraday constant 96485 C/mol , and Q is the reaction quotient.For the reaction quotient Q , we have:Q = [Ag]/[Cu] = 0.1 M / 0.5 M = 0.02Now, we can plug in the values into the Nernst equation:E = 0.46 V - 8.314 J/molK * 298.15 K / 2 * 96485 C/mol * ln 0.02 E 0.46 V - 0.0129 V * ln 0.02 E 0.46 V - 0.0129 V * -3.912 E 0.46 V + 0.0505 VE 0.5105 VThe polarization of the cell is the difference between the measured potential difference and the calculated cell potential:Polarization = Measured potential - Calculated potentialPolarization = 0.75 V - 0.5105 VPolarization 0.2395 V