To calculate the standard enthalpy change of reduction for the given reaction, we can use the relationship between the standard electrode potential E and the standard Gibbs free energy change G as follows:G = -nFEwhere n is the number of moles of electrons transferred in the reaction in this case, 2 , F is the Faraday constant approximately 96,485 C/mol , and E is the standard electrode potential.First, we need to find the G for the reduction of Cu2+ aq to Cu s using the given standard electrode potential:G = -nFEG = - 2 mol 96,485 C/mol +0.34 V G = -65,609.8 J/molNow, we can use the relationship between G, H standard enthalpy change , and S standard entropy change to find H:G = H - TSAt standard conditions, the temperature T is 298.15 K. However, we don't have the value for S. In many cases, the entropy change is relatively small compared to the enthalpy change, so we can make an approximation by assuming that G H. This is not always accurate, but it can give us a rough estimate of the standard enthalpy change of reduction:H GH -65,609.8 J/molTherefore, the approximate standard enthalpy change of reduction for the reaction Cu2+ aq + 2e- -> Cu s is -65,609.8 J/mol.