To calculate the standard electrode potential of the given cell reaction, we can use the Nernst equation. First, we need to know the standard reduction potentials for the half-reactions:Cu2+ + 2e- Cu s E Cu2+/Cu = +0.34 VZn2+ + 2e- Zn s E Zn2+/Zn = -0.76 VThe overall cell reaction is:Cu2+ + Zn s Cu s + Zn2+Now, we can use the Nernst equation to find the electrode potential E at the given concentrations:E = E cell - RT/nF * ln Q where E cell is the standard cell potential, R is the gas constant 8.314 J/molK , T is the temperature in Kelvin 25C = 298.15 K , n is the number of electrons transferred 2 in this case , F is the Faraday constant 96485 C/mol , and Q is the reaction quotient.First, we need to find E cell :E cell = E Cu2+/Cu - E Zn2+/Zn = 0.34 V - -0.76 V = 1.10 VNow, we can calculate Q:Q = [Zn2+]/[Cu2+] = 1.0 M / 0.01 M = 100Now, we can plug these values into the Nernst equation:E = 1.10 V - 8.314 J/molK * 298.15 K / 2 * 96485 C/mol * ln 100 E = 1.10 V - 0.0257 V * ln 100 E = 1.10 V - 0.0257 V * 4.605E 1.10 V - 0.118 VE 0.982 VSo, the standard electrode potential of the given cell reaction at 25C is approximately 0.982 V.