Chapter 17, Problem 17.35CP

Consider the following table of standard reduction potentials:

Reduction Half-Reaction	E° (V)
${\text{A}}^{+}+{\text{e}}^{-}\to \text{A}$	0.80
${\text{B}}^{\text{2+}}+2{\text{e}}^{-}\to \text{B}$	0.38
${\text{C}}_2+2{\text{e}}^{-}\to 2{\text{C}}^{-}$	0.17
${\text{D}}^{3+}+3{\text{e}}^{-}\to \text{D}$	–1.36

1. (a) Which substance is the strongest oxidizing agent? Which is the strongest reducing agent?
2. (b) Which substances can be oxidized by B²⁺? Which can be reduced by D?
3. (c) Write a balanced equation for the overall cell reaction that delivers a voltage of 1.53 V under standard-state conditions.