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Number of moles of MnO4^- required to oxidize one mole of ferrous oxalate completely in acidic medium will be:

1. 6 moles
2. 0.4 moles
3. 7.5 moles
4. 0.2 moles

Correct answer: 0.4 moles

Solution

The balanced chemical equation for the oxidation of ferrous oxalate is 2MnO4^- + 5FeC2O4 + 16H+ -> 2Mn^2+ + 10CO2 + 8H2O. From the equation, 2 moles of MnO4^- are required to oxidize 5 moles of ferrous oxalate. Therefore, 1 mole of MnO4^- is required to oxidize 2.5 moles of ferrous oxalate, and 0.4 moles of MnO4^- are required to oxidize 1 mole of ferrous oxalate.

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