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_2O_4^(2-))) + 24H^(+) to 3Mn^(2+) + 5Fe^(3+) + 10 CO_2 + 12 H_2O`
Thus 5M of `FeC_2O_4` is oxidised by 3M of `KMnO_4` then 1M of `FeC_2O_4` is oxidised by 3/5 mole of `KMnO_4`.