Question

Given the following reaction at standard conditions:Cu(s) + 2Ag+(aq) -> Cu2+(aq) + 2Ag(s) Calculate the cell potential, E°cell, at 25°C using the standard reduction potentials:Cu2+(aq) + 2e- -> Cu(s), E°red = +0.34 VAg+(aq) + e- -> Ag(s), E°red = +0.80 V

Answer 1

To calculate the cell potential  Ecell  for the given reaction, we need to determine the reduction and oxidation half-reactions. The given standard reduction potentials are:Cu2+ aq  + 2e- -> Cu s , Ered = +0.34 V  reduction Ag+ aq  + e- -> Ag s , Ered = +0.80 V  reduction Since Cu s  is being oxidized to Cu2+ aq  in the overall reaction, we need to reverse the first half-reaction:Cu s  -> Cu2+ aq  + 2e-, Eox = -0.34 V  oxidation Now, we can combine the oxidation and reduction half-reactions:Cu s  -> Cu2+ aq  + 2e-  oxidation 2 Ag+ aq  + e- -> Ag s    reduction, multiplied by 2 to balance electrons The overall reaction is:Cu s  + 2Ag+ aq  -> Cu2+ aq  + 2Ag s Now, we can calculate the cell potential  Ecell  using the Nernst equation:Ecell = Ered reduction  - Eox oxidation Ecell =  +0.80 V  -  -0.34 V  = 0.80 V + 0.34 V = 1.14 VSo, the cell potential  Ecell  for the given reaction at 25C is 1.14 V.