Oxidation-Reduction

38) The reason for each of the choices below is the same. The more readily a substance is reduced (the more positive the E°_red or the more negative the E°_ox ) the stronger the oxidizing agent.

      (a) Ce⁴⁺(aq) + e^- Ce³⁺(aq)                            E°_red = +1.61 V

           Br₂(l) + 2e^- 2Br^-(aq)                                 E°_red = +1.065 V

           H₂O₂(aq) + 2H⁺(aq) + 2e^- 2H₂O(l)          E°_red = +1.776 V

           Zn(s) + 2e^-                                                             E°_red = ??? (Zn is not very likely to be reduced.)

           H₂O₂(aq) is the strongest oxidizing agent and Zn(s) is the weakest.

      (b) F₂(g) + 2e^- 2F^-(aq)                                                 E°_red = +2.87 V

           Zn²⁺(aq) + 2e^- Zn(s)                                               E°_red = -0.763 V

           N₂(g) + 5H⁺(aq) + 4e^- N₂H₅⁺(aq)                          E°_red = -0.23 V

           I₂(s) + 2e^- 2I^-(aq)                                                    E°_red = +0.536 V

           NO₃^-(aq) + 4H⁺(aq) + 3e^- NO(g) + 2H₂O(l)          E°_red = +0.96 V

           Zn(s) is the strongest reducing agent and F^- is the weakest.