Write the formula of the strongest oxidizing agent given the following standard reduction potentials in acid solution: $\begin{array}{ll}
\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.23 \mathrm{~V} \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & \mathrm{E}^{\circ}=+0.13 \mathrm{~V} \
\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{~s}) & \mathrm{E}^{\circ}=-0.76 \mathrm{~V}
\end{array}$

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The Answer of Write the formula of the strongest oxidizing agent given the following standard reduction potentials in acid solution: $\begin{array}{ll}
\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.23 \mathrm{~V} \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & \mathrm{E}^{\circ}=+0.13 \mathrm{~V} \
\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{~s}) & \mathrm{E}^{\circ}=-0.76 \mathrm{~V}
\end{array}$

Write the Formula of the Strongest Oxidizing Agent Given the Following