Chapter 17.5, Problem 17.9CP

Consider the following table of standard reduction potentials:

Reduction Half-Reaction	E°(V)
${\text{A}}^{3+}+2{\text{e}}^{-}\to {\text{A}}^{+}$	1.47
${\text{B}}^{\text{2+}}+2{\text{e}}^{-}\to \text{B}$	0.60
${\text{C}}^{\text{2+}}+2{\text{e}}^{-}\to \text{C}$	–0.21
${\text{D}}^{+}+{\text{e}}^{-}\to \text{D}$	–1.38

1. (a) Which substance is the strongest reducing agent? Which is the strongest oxidizing agent?
2. (b) Which substances can be oxidized by B²⁺? Which can be reduced by C?
3. (c) Write a balanced equation for the overall cell reaction that delivers the highest voltage, and calculate E° for the reaction.