The document details a redox reaction involving nitrate ions and hydrogen ions producing nitrogen dioxide and water. It presents the reduction potential (ered) of +0.80 V and the oxidation potential (eox) of -0.34 V for copper, resulting in a cell potential (ecell) of +0.46 V. The overall summary highlights the conversion processes of the reactants and the associated electrode potentials.

1. NO3-(aq) + 2H+(aq) + e- ---> NO2(g) + H2O(l) Ered = +0.80 V
Cu(s) ---> Cu2+(aq) + 2e- Eox = -0.34 v
Ecell = Eox + Ered = 0.80 - 0.34 = + 0.46 V
Solution
NO3-(aq) + 2H+(aq) + e- ---> NO2(g) + H2O(l) Ered = +0.80 V
Cu(s) ---> Cu2+(aq) + 2e- Eox = -0.34 v
Ecell = Eox + Ered = 0.80 - 0.34 = + 0.46 V