To calculate the corrosion potential of the copper metal electrode, we can use the Nernst equation. The Nernst equation relates the reduction potential of an electrochemical reaction to the standard electrode potential, temperature, and the activities of the chemical species involved in the reaction. For the Cu2+/Cu electrode, the half-cell reaction is:Cu2+ + 2e- -> CuThe Nernst equation for this reaction is:E = E - RT/nF * ln Q where E is the corrosion potential, E is the standard electrode potential, R is the gas constant 8.314 J/molK , T is the temperature in Kelvin 298 K , n is the number of electrons transferred in the reaction 2 for Cu2+/Cu , F is the Faraday constant 96485 C/mol , and Q is the reaction quotient.In this case, E = +0.34 V, and the reaction quotient Q is given by:Q = [Cu]/[Cu2+]Since the copper metal electrode is in its standard state, its activity is 1. The concentration of Cu2+ ions in the solution is 0.1 M. Therefore, Q = 1/0.1 = 10.Now we can plug these values into the Nernst equation:E = 0.34 - 8.314 * 298 / 2 * 96485 * ln 10 E = 0.34 - 0.043 / 2 * ln 10 E = 0.34 - 0.0215 * 2.303E = 0.34 - 0.0495E = 0.2905 VThe corrosion potential of the copper metal electrode in the given solution is approximately +0.2905 V with respect to the hydrogen electrode.