Electrode potentials $\left(\mathrm{E}^{\circ}\right)$ are given below : $\begin{aligned} & \mathrm{Cu}^{+}…
Electrode potentials $\left(\mathrm{E}^{\circ}\right)$ are given below :
$\begin{aligned}
& \mathrm{Cu}^{+} / \mathrm{Cu}=+0.52 \mathrm{~V} ,\\
& \mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}=+0.77 \mathrm{~V}, \\
& \frac{1}{2} \mathrm{I}_2(\mathrm{~s}) / \mathrm{I}^{-}=+0.54 \mathrm{~V}, \\
& \mathrm{Ag}^{+} / \mathrm{Ag}=+0.88 \mathrm{~V}.
\end{aligned}$
Based on the above potentials, strongest oxidizing agent will be :
$\mathrm{Cu}^{+}$
$\mathrm{Fe}^{3+}$
$\mathrm{Ag}^{+}$
$\mathrm{I}_2$
Solution
Higher the value of reduction potential stronger will be the oxidising hence based on the given values $\mathrm{Ag}^{+}$will be strongest oxidizing agent.