To calculate the corrosion potential of the zinc electrode, we can use the Nernst equation. The Nernst equation relates the reduction potential of a half-cell at any point in time to the standard electrode potential, temperature, and the activities of the chemical species involved.For the zinc half-cell, the Nernst equation is:E_Zn = E_Zn - RT/nF * ln Q For the copper half-cell, the Nernst equation is:E_Cu = E_Cu - RT/nF * ln Q Where:E_Zn and E_Cu are the reduction potentials of the zinc and copper half-cells, respectivelyE_Zn = -0.76 V standard reduction potential for Zn2+ E_Cu = +0.34 V standard reduction potential for Cu2+ R = 8.314 J/ molK gas constant T = 25C = 298.15 K temperature in Kelvin n = 2 number of electrons transferred in each half-reaction F = 96485 C/mol Faraday's constant Q is the reaction quotient, which is equal to the concentration of the reduced species divided by the concentration of the oxidized speciesSince the concentrations of Zn2+ and Cu2+ are both 0.1 M, the reaction quotient Q for both half-cells is equal to 1. Therefore, ln Q = ln 1 = 0, and the Nernst equation simplifies to:E_Zn = E_ZnE_Cu = E_CuNow, we can calculate the overall cell potential corrosion potential , which is the difference between the reduction potentials of the two half-cells:E_cell = E_Cu - E_Zn = +0.34 V - -0.76 V = +1.10 VThe corrosion potential of the zinc electrode in this system is +1.10 V.