The more positive the value of ${\mathrm{E}}^{⊝}$, the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.

1. Fe3+

2. I2(s)

3. Cu2+

4. Ag+

Hint: High reduction potential value strongest is the oxidisng agent

The given values are as follows:

$\mathrm{E}°$ values of

${\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}=+0.77\mathrm{V}\phantom{\rule{0ex}{0ex}}{\mathrm{I}}_{2}\left(\mathrm{s}\right)/{\mathrm{I}}^{-}=+0.54\mathrm{V}\phantom{\rule{0ex}{0ex}}{\mathrm{Cu}}^{2+}/\mathrm{Cu}=+0.34\mathrm{V}\phantom{\rule{0ex}{0ex}}{\mathrm{Ag}}^{+}/\mathrm{Ag}=+0.80\mathrm{V}$

Since, $\mathrm{E}°$ of the redox couple ${\mathrm{Ag}}^{+}/\mathrm{Ag}$ is the most positive, i.e., 0.80 V, therefore Ag+ is the strongest oxidising agent.