To calculate the activation energy for the oxidation of copper, we can use the Tafel equation, which relates the overpotential to the exchange current density i0 and the current density i of the electrochemical reaction: = RT/nF * ln i/i0 where R is the gas constant 8.314 J/molK , T is the temperature 298 K , n is the number of electrons transferred 2 for the Cu/Cu2+ redox couple , and F is the Faraday constant 96485 C/mol .First, we need to find the current density i for the reaction. We can use the Nernst equation to find the equilibrium potential E for the reaction:E = E - RT/nF * ln [Cu2+]/[Cu] Since the reaction order is unity, the concentrations of Cu2+ and Cu are equal, so the ln term becomes ln 1 = 0. Therefore, the equilibrium potential is equal to the standard reduction potential:E = +0.34 VNow, we can use the Butler-Volmer equation to find the current density i :i = i0 * exp nF/RT - exp -nF/RT Since the reaction is at equilibrium, the net current density i is zero:0 = i0 * exp nF/RT - exp -nF/RT We can rearrange the equation to solve for the overpotential : = RT/nF * ln exp -nF/RT Now, we can plug in the values for R, T, n, F, and i0: = 8.314 J/molK * 298 K / 2 * 96485 C/mol * ln 5.6 x 10^-6 Acm^-2 0.0429 VFinally, we can use the Arrhenius equation to find the activation energy Ea :Ea = * n * FEa = 0.0429 V * 2 * 96485 C/molEa 8260 J/molSo, the activation energy for the oxidation of copper in a 1 M copper sulfate solution is approximately 8260 J/mol.