Use the Following Standard Reduction Potentials to Determine Which Species

question 15

Multiple Choice

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

• A) I₂(s)
• B) O₂(g)
• C) I^-(aq)
• D) Hg₂²⁺(aq)
• E) H₂O( \(\ell\) )

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