The number of mole of `KMnO_(4)` that will be needed to react completely with one mole of ferrous oxalate in acidic solution is:
A
`3//5`
B
`2//5`
C
`4//5`
D
1
Text Solution
Verified by Experts
The correct Answer is:
A
`3underset(3M)MnO_(4)^(-) + 5 (Fe^(2+) underset(5M) + C_(2)O_(4)^(2-)) + 24H^(+) rarr 3 Mn^(2) + 5 Fe^(3+) + 10 O_(2) + 12 H_(2) O` Thus `5M` of `FeC_(2)O` is oxidised by `3M` of `KMn_(2) O_(2)` the `1M` of `FeC_(2)O_(4)` is oxidised by `3//5` mole of `KMn_(2)O`.
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