Given the list of reduction potentials, which of the following species is the strongest reducing agent?
Li+(aq)+ e– →Li (s) Eored = -3.04 V
Zn2+(aq) + 2 e– → Zn (s) Eored = -0.76 V
Ag+(aq) + e– → Ag (s) Eored = 0.80 V
Ce4+(aq) + e– → Ce3+ (s) Eored = 1.44 V
This question is testing your understanding of the redox chemistry and reduction potentials. To answer this question, you must first know that a reducing agent is itself oxidized. Therefore, the strongest reducing agent is going to be the species that is most readily oxidized. The Nernst equation, DG = -nFE, shows that a spontaneous reaction (DG < 0) corresponds to an electrochemical potential, E, that is greater than zero.
Since Ce4+ is spontaneously reduced, choice A can be eliminated. Zn2+ is already in its oxidized form and therefore cannot be oxidized further making B the wrong answer. Considering answer choices C and D, you must reverse the reactions to find Eoox, which equals the negative of the reduction potential (Eoox = -Eored). Therefore, the oxidation of Ag(s) is a nonspontaneous reaction while the oxidation of Li(s) proceeds spontaneous with a potential of +3.04 V, making C the correct answer.