The number of moles of `KMnO_(4)` that will be needed to react completely with one mole of ferrous oxalate in acidic solution is:

Options

A. `3//5`
B. `2//5`
C. `4//5`
D. 1

Answer

A

Explanation

`underset(3M)(3MnO_(4)^(-))+underset(5M)(5(Fe^(2+)+C_(2)O_(4)^(2-)))+23H^(+)rarr3Mn^(2+)+5Fe^(3+)+10CO_(2)+12H_(2)O`
Thus 5M of `FeC_(2)O_(4)` is oxidation by 3M of `KMnO_(4)` then 1M of `FeC_(2)O_(4)` is oxidation by `3//5` mole of `KMnO_(4)`.