Use the Table of Standard Reduction Potentials Below to Identify

Use the table of standard reduction potentials below to identify the metal or metal ion that is the strongest reducing agent. Standard Reduction Potentials (volts) in Aqueous
Solution
$$\begin{array} { l l } \mathrm { Pb } ^ { 4 + } + 2 \mathrm { e } ^ { - } \rightarrow \mathrm { Pb } ^ { 2 + } & + 1.80 \\\mathrm { Au } ^ { 3 + } + 3 \mathrm { e } ^ { - } \rightarrow \mathrm { Au } & + 1.50 \\\mathrm { Fe } ^ { 3 + } + 3 \mathrm { e } ^ { - } \rightarrow \mathrm { Fe } & + 0.771 \\\mathrm { I } _ { 2 } + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { I } ^ { - } & + 0.535 \\\mathrm {~Pb} ^ { 2 + } + 2 \mathrm { e } ^ { - } \rightarrow \mathrm { Pb } & - 0.124 \\\mathrm { Al } ^ { 3 + } + 3 \mathrm { e } ^ { - } \rightarrow \mathrm { Al } & - 1.66 \\\mathrm { Mg } ^ { 2 + } + 2 \mathrm { e } ^ { - } \rightarrow \mathrm { Mg } & - 2.37 \\\mathrm {~K} ^ { + } + \mathrm { e } ^ { - } \rightarrow \mathrm { K } & - 2.93\end{array}$$

A) Pb⁴⁺
B) Pb²⁺
C) K⁺
D) K
E) Al