To calculate the standard cell potential for a galvanic cell made up of a silver electrode and a zinc electrode, we need to use the Nernst equation. The Nernst equation relates the cell potential E_cell to the standard cell potential E_cell , temperature T , number of electrons transferred n , the gas constant R , and the concentrations of the ions involved in the redox reaction.The Nernst equation is:E_cell = E_cell - RT/nF * ln Q where:E_cell = standard cell potentialR = gas constant 8.314 J/molK T = temperature in Kelvin, 298 K for standard conditions n = number of electrons transferredF = Faraday's constant 96,485 C/mol Q = reaction quotientFirst, we need to find the standard cell potential E_cell for the given redox reaction. The half-cell reactions for silver and zinc are:Ag aq + e Ag s E = +0.80 V reduction Zn aq + 2e Zn s E = -0.76 V reduction Since zinc is being oxidized and silver is being reduced, we need to reverse the zinc half-cell reaction:Zn s Zn aq + 2e E = +0.76 V oxidation Now, we can find the standard cell potential by adding the half-cell potentials:E_cell = E Ag/Ag + E Zn/Zn = +0.80 V + +0.76 V = +1.56 VNext, we need to find the reaction quotient Q . The balanced redox reaction is:2Ag aq + Zn s 2Ag s + Zn aq The reaction quotient Q is given by:Q = [Zn]/[Ag]^2Given the concentrations of silver ions 0.01 M and zinc ions 1.0 M , we can calculate Q:Q = 1.0 M / 0.01 M ^2 = 10000Now, we can use the Nernst equation to find the cell potential E_cell :E_cell = E_cell - RT/nF * ln Q E_cell = 1.56 V - 8.314 J/molK * 298 K / 2 * 96485 C/mol * ln 10000 E_cell 1.56 V - 0.0296 V * ln 10000 E_cell 1.56 V - 0.0296 V * 9.21E_cell 1.56 V - 0.272E_cell 1.288 VSo, the standard cell potential for a galvanic cell made up of a silver electrode and a zinc electrode with the given concentrations of ions is approximately 1.288 V.