To calculate the cell potential for the given electrochemical reaction, we need to find the difference in standard reduction potentials between the two half-reactions. The reaction is:Zn s + Cu aq Zn aq + Cu s The half-reactions are:Zn s Zn aq + 2e oxidation Cu aq + 2e Cu s reduction Given standard reduction potentials are:E Zn/Zn = -0.76 VE Cu/Cu = +0.34 VSince Zn is being oxidized, we need to reverse the sign of its standard reduction potential to get the standard oxidation potential:E Zn/Zn = +0.76 VNow, we can calculate the cell potential Ecell using the formula:Ecell = Ecathode - EanodeIn this case, Cu/Cu is the cathode reduction and Zn/Zn is the anode oxidation :Ecell = +0.34 V - +0.76 V = -0.42 VHowever, since the cell potential should be positive for a spontaneous reaction, we need to reverse the reaction:Zn aq + Cu s Zn s + Cu aq Now the half-reactions are:Zn aq + 2e Zn s reduction Cu s Cu aq + 2e oxidation And the standard reduction potentials are:E Zn/Zn = -0.76 VE Cu/Cu = -0.34 VNow, we can calculate the cell potential Ecell using the formula:Ecell = Ecathode - EanodeIn this case, Zn/Zn is the cathode reduction and Cu/Cu is the anode oxidation :Ecell = -0.76 V - -0.34 V = 0.42 VSo, the cell potential for the given electrochemical reaction at 25C is 0.42 V.