Oxidation of FeC2O4
In acidic medium, both K2Cr2O7 (potassium dichromate) and KMnO4 (potassium permanganate) can act as strong oxidizing agents. To determine the number of moles required to oxidize one mole of FeC2O4, we need to understand the oxidation states and the reactions involved.
1. Reaction with K2Cr2O7
- The oxidation half-reaction for FeC2O4 involves converting Fe(II) to Fe(III) and oxidizing oxalate ions (C2O4) to CO2.
- The balanced equation shows that 1 mole of K2Cr2O7 can oxidize 6 moles of electrons.
- Since oxidizing 1 mole of FeC2O4 releases 2 moles of electrons, the number of moles of K2Cr2O7 required is:
- 2 moles of electrons / 6 moles of electrons per mole of K2Cr2O7 = 1/3.
- Therefore, 1 mole of K2Cr2O7 is required to oxidize 3 moles of FeC2O4.
2. Reaction with KMnO4
- The oxidation half-reaction with KMnO4 involves the conversion of Fe(II) to Fe(III) and the oxidation of oxalate ions as well.
- For KMnO4, 1 mole can accept 5 moles of electrons.
- Since the oxidation of 1 mole of FeC2O4 also involves 2 moles of electrons, the moles of KMnO4 required is:
- 2 moles of electrons / 5 moles of electrons per mole of KMnO4 = 2/5.
- Thus, 5 moles of KMnO4 are required to oxidize 2 moles of FeC2O4.
Summary
- K2Cr2O7: 1 mole required for 3 moles of FeC2O4.
- KMnO4: 5 moles required for 2 moles of FeC2O4.