Use the following standard reduction potentials to determine which species is the best oxidizing agent.
$$\begin{array} { l l }
\mathrm { O } _ { 2 } ( \mathrm {~g} ) + 4 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 4 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) & E ^ { \circ } = + 1.229 \mathrm {~V} \
\mathrm {{ Hg } _ { 2 }} ^ { 2 + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { Hg } ( \ell ) & E ^ { \circ } = + 0.789 \mathrm {~V} \
\mathrm { I } _ { 2 } ( \mathrm {~s} ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { I } ^ { - } ( \mathrm { aq } ) & E ^ { \circ } = + 0.535 \mathrm {~V}
\end{array}$$

Question

Use the following standard reduction potentials to determine which species is the best oxidizing agent. 
$$\begin{array} { l l } 
\mathrm { O } _ { 2 } ( \mathrm {~g} ) + 4 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 4 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) & E ^ { \circ } = + 1.229 \mathrm {~V} \
\mathrm {{ Hg } _ { 2 }} ^ { 2 + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { Hg } ( \ell ) & E ^ { \circ } = + 0.789 \mathrm {~V} \
\mathrm { I } _ { 2 } ( \mathrm {~s} ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { I } ^ { - } ( \mathrm { aq } ) & E ^ { \circ } = + 0.535 \mathrm {~V}
\end{array}$$

Quizplus · Accepted Answer

The standard reduction potential of O₂(g) is the highest, indicating that it is the best oxidizing agent among the given species.

Use the Following Standard Reduction Potentials to Determine Which Species