To calculate the cell potential at standard conditions for the given electrochemical reaction, we first need to identify the reduction and oxidation half-reactions. The given standard reduction potentials are:Cu2+ aq + 2e- -> Cu s E = +0.34 V reduction Ag+ aq + e- -> Ag s E = +0.80 V reduction In the overall reaction, Cu s is being oxidized to Cu2+ aq , so we need to reverse the first half-reaction to get the oxidation half-reaction:Cu s -> Cu2+ aq + 2e- E = -0.34 V oxidation Now, we need to balance the electrons in both half-reactions. Since the second half-reaction involves only one electron, we need to multiply it by 2 to balance the electrons with the first half-reaction:2 Ag+ aq + e- -> Ag s E = 2 +0.80 V = +1.60 V reduction Now, we can add the two balanced half-reactions to get the overall reaction:Cu s -> Cu2+ aq + 2e- E = -0.34 V oxidation 2Ag+ aq + 2e- -> 2Ag s E = +1.60 V reduction ----------------------------------------------Cu s + 2Ag+ aq -> 2Ag s + Cu2+ aq Finally, we can calculate the cell potential Ecell at standard conditions by adding the standard potentials of the oxidation and reduction half-reactions:Ecell = E reduction + E oxidation Ecell = +1.60 V + -0.34 V Ecell = +1.26 VSo, the cell potential at standard conditions for the given electrochemical reaction is +1.26 V.