To find the cell potential for the reaction, we need to determine which half-reaction will act as the anode oxidation and which will act as the cathode reduction . The half-reaction with the lower standard reduction potential will act as the anode, and the half-reaction with the higher standard reduction potential will act as the cathode.In this case, the Cu/Cu half-reaction has a lower standard reduction potential E = +0.34 V compared to the Ag/Ag half-reaction E = +0.80 V . Therefore, the Cu/Cu half-reaction will act as the anode oxidation and the Ag/Ag half-reaction will act as the cathode reduction .Now, we need to reverse the anode half-reaction to represent oxidation:Cu s Cu aq + 2eThe cell potential Ecell can be calculated by subtracting the standard reduction potential of the anode Eanode from the standard reduction potential of the cathode Ecathode :Ecell = Ecathode - EanodeEcell = +0.80 V - +0.34 V Ecell = +0.46 VThe cell potential for the reaction when a copper electrode is paired with a silver electrode in a standard electrochemical cell is +0.46 V.