Using the standard electrode potentials of the redox couples given below, which of the following is the strongest oxidizing agent?

${\mathrm{E}}^{⊝} \mathrm{values}: {\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}=+0.\mathrm{77\; V}$ 
${\mathrm{I}}_2\left(\mathrm{s}\right)/{\mathrm{I}}^{-}=+0.54 V$
${\mathrm{Cu}}^{2+}/\mathrm{Cu}=+0.\mathrm{34\; V}$
${\mathrm{Ag}}^{+}/\mathrm{Ag}=0.\mathrm{80\; V}$

1. Fe³⁺
2. I₂(s)
3. Cu²⁺
4. Ag⁺

Using the standard electrode potential, find out the pair between which redox reaction is not feasible.

${\mathrm{E}}^{⊝} \mathrm{values}: {\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}=+0.77; {\mathrm{I}}_2/{\mathrm{I}}^{-}=+0.54;$
${\mathrm{Cu}}^{2+}/\mathrm{Cu}=+0.34; {\mathrm{Ag}}^{+}/\mathrm{Ag}=+0.80 \mathrm{V}$

1. Fe³⁺ and I^-

2. Ag⁺ and Cu

3. Fe³⁺ and Cu

4. Ag and Fe³⁺