To calculate the corrosion potential and determine which electrode will corrode and which will act as a cathode, we need to find the cell potential E_cell for the galvanic cell. The cell potential can be calculated using the standard reduction potentials of the two half-cells.E_cell = E_cathode - E_anodeSince we want the cell potential to be positive spontaneous reaction , we need to choose the half-cell with the higher reduction potential as the cathode and the one with the lower reduction potential as the anode.In this case, the standard reduction potentials are:Cu2+/Cu: +0.34 VAg+/Ag: +0.80 VSince the reduction potential of Ag+/Ag is higher than that of Cu2+/Cu, the silver electrode will act as the cathode, and the copper electrode will act as the anode.Now, we can calculate the cell potential:E_cell = E_cathode - E_anodeE_cell = +0.80 V - +0.34 V E_cell = +0.46 VThe corrosion potential of the copper electrode immersed in a 1 M CuSO4 solution in contact with a silver electrode immersed in a 1 M AgNO3 solution is +0.46 V. The copper electrode will corrode act as the anode , and the silver electrode will act as the cathode.