To calculate the standard cell potential for this galvanic cell, we need to use the Nernst equation. The Nernst equation is given by: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 assuming 298 K for room temperature , n is the number of electrons transferred in the redox reaction, F is the Faraday constant 96485 C/mol , and Q is the reaction quotient.First, we need to determine the standard cell potential, E_cell. The standard reduction potentials for silver and copper are:Ag + e Ag s E = +0.80 VCu + 2e Cu s E = +0.34 VSince the silver electrode is the cathode reduction occurs and the copper electrode is the anode oxidation occurs , we can write the overall cell reaction as:2Ag + Cu s 2Ag s + CuNow, we can calculate the standard cell potential, E_cell, by subtracting the standard reduction potential of the anode from the standard reduction potential of the cathode:E_cell = E_cathode - E_anode = 0.80 V - 0.34 V = 0.46 VNext, we need to determine the reaction quotient, Q. For the given reaction, Q is given by:Q = [Cu]/[Ag]^2Plugging in the given concentrations:Q = 0.1 M / 0.05 M ^2 = 0.1/0.0025 = 40Now, we can use the Nernst equation to calculate the cell potential, E_cell:E_cell = E_cell - RT/nF * ln Q E_cell = 0.46 V - 8.314 J/molK * 298 K / 2 * 96485 C/mol * ln 40 Converting R to V by dividing by 1000:E_cell = 0.46 V - 0.008314 V/molK * 298 K / 2 * 96485 C/mol * ln 40 E_cell = 0.46 V - 0.00247 V * ln 40 E_cell 0.46 V - 0.00247 V * 3.6889E_cell 0.46 V - 0.0091 VE_cell 0.4509 VTherefore, the standard cell potential for this galvanic cell is approximately 0.4509 V.