For the balanced equation : 

$$\begin{gathered} 8{\mathrm{H}}^{+}\left(aq\right)+5{\mathrm{Fe}}^{2+}\left(aq\right)+{\mathrm{MnO}}_4^{-}\left(aq\right) \\ ⟶5{\mathrm{Fe}}^{3+}\left(aq\right)+{\mathrm{Mn}}^{2+}\left(aq\right)+4{\mathrm{H}}_2\mathrm{O}\left(l\right) \end{gathered}$$

Which statement is correct?

The reaction is,

$8{\mathrm{H}}^{+}\left(aq\right)+5{\mathrm{Fe}}^{2+}\left(aq\right)+{\mathrm{MnO}}_4^{-}\left(aq\right)\to 5{\mathrm{Fe}}^{3+}\left(aq\right)+{\mathrm{Mn}}^{2+}\left(aq\right)+4{\mathrm{H}}_2\mathrm{O}\left(l\right)$Since acidified manganate (VII) ions are potent oxidizers. They are able to convert  ${\mathrm{Fe}}^{2+}$ ion into ${\mathrm{Fe}}^{3+}$ ions as a result  ${\mathrm{Fe}}^{2+}\left(aq\right)$ undergoes oxidation.

Hence, option A is correct.