One mole of ${\mathrm{KMnO}}_4$ is used for complete oxidation of ${\mathrm{FeSO}}_4,{\mathrm{FeC}}_2{\mathrm{O}}_4$ and ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4$ respectively (and separately). Pick up the correct statement :

The reaction is, 

(I)  ${\stackrel{+7}{\mathrm{KMnO}}}_4^{ }\stackrel{{\mathrm{H}}^{+}}{⟶}{\mathrm{Mn}}^{+2}-5e^{-}$

(II) ${\mathrm{Fe}}^{+2}+{\mathrm{C}}_2^{+3}{\mathrm{O}}_4^{-2}⟶2{\mathrm{CO}}_2^{+2}+{\mathrm{Fe}}^{+3}+3e$

(III)  ${\mathrm{H}}_2{\mathrm{C}}_2\stackrel{+3}{{\mathrm{O}}_4^{ }}⟶\stackrel{+4}{2{\mathrm{CO}}_2^{ }}+2e^{-}$

(A) 5 mole of ${\mathrm{FeSO}}_4$ can be oxidised

(B) $\frac{5}{3}$ mole of ${\mathrm{FeC}}_2{\mathrm{O}}_4$ can be oxidised

(C) 2.5 mole of ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4$can be oxidised

Thus, correct options are A, C and D.