To calculate the corrosion potential of the zinc rod in a galvanic couple with a standard hydrogen electrode, we need to consider the half-cell reactions and the Nernst equation.The half-cell reactions are:Zn s Zn aq + 2e E = -0.76 V Cu aq + 2e Cu s E = +0.34 V The overall reaction is:Zn s + Cu aq Zn aq + Cu s The cell potential E_cell is the difference between the reduction potential of the cathode copper and the anode zinc :E_cell = E Cu/Cu - E Zn/Zn = 0.34 V - -0.76 V = 1.10 VNow we need to apply the Nernst equation to account for the non-standard conditions 0.1 M Cu :E = E - RT/nF * ln Q Where:E = corrosion potentialE = standard cell potentialR = gas constant 8.314 J/molK T = temperature in Kelvin 25C = 298 K n = number of electrons transferred 2 for this reaction F = Faraday's constant 96485 C/mol Q = reaction quotient = [Zn]/[Cu]Since the zinc rod is being placed in the solution, we can assume that [Zn] is negligible compared to [Cu]. Therefore, Q 1/[Cu] = 1/0.1 = 10.Now we can plug in the values:E = 1.10 V - 8.314 J/molK * 298 K / 2 * 96485 C/mol * ln 10 E = 1.10 V - 0.0257 V * ln 10 E = 1.10 V - 0.0592 VE 1.04 VThe corrosion potential of the zinc rod in a galvanic couple with a standard hydrogen electrode at 25C is approximately 1.04 V.