To calculate the corrosion potential of a zinc-copper galvanic couple, we can use the Nernst equation. The Nernst equation relates the reduction potential of a half-cell at non-standard conditions to the standard reduction potential, temperature, and reaction quotient.E = E - RT/nF * ln Q where:E = reduction potential at non-standard conditionsE = standard reduction potentialR = gas constant 8.314 J/molK T = temperature in Kelvin assume 298 K for room temperature n = number of electrons transferred in the redox reaction 2 for both Zn and Cu redox reactions F = Faraday's constant 96485 C/mol Q = reaction quotient, which is the ratio of the concentrations of the products to the reactantsFor the zinc half-cell oxidation :Zn s -> Zn aq + 2eE Zn = -0.76 VFor the copper half-cell reduction :Cu aq + 2e -> Cu s E Cu = +0.34 VThe overall reaction is:Zn s + Cu aq -> Zn aq + Cu s Now, we can calculate the corrosion potential E_corr using the Nernst equation for both half-cells and then subtracting the two potentials.For the zinc half-cell:E Zn = E Zn - RT/2F * ln [Zn]/1 E Zn = -0.76 - 8.314 * 298 / 2 * 96485 * ln 0.1 E Zn -0.76 + 0.0295E Zn -0.7305 VFor the copper half-cell:E Cu = E Cu - RT/2F * ln 1/[Cu] E Cu = +0.34 - 8.314 * 298 / 2 * 96485 * ln 1/0.01 E Cu +0.34 + 0.059E Cu +0.399 VNow, we can calculate the corrosion potential E_corr for the zinc-copper galvanic couple:E_corr = E Cu - E Zn E_corr = +0.399 - -0.7305 E_corr +1.1295 VThe corrosion potential of the zinc-copper galvanic couple is approximately +1.1295 V.