Permanganate Oxidation of Iron(II)
MnO4− + 5Fe2+ + 8H+ → Mn2+ + 5Fe3+ + 4H2O
Overview
Permanganate ion is a powerful oxidizing agent that oxidizes iron(II) to iron(III) while being reduced from Mn(VII) to Mn(II) in acidic solution. The dramatic color change from deep purple KMnO₄ to nearly colorless Mn²⁺ makes this reaction self-indicating in titrations.
Participants
| Role | Substance | Coefficient | State |
|---|---|---|---|
| Product | Water H₂O | 4 | (l) |
Everyday Example
Potassium permanganate's purple color is used in water purification systems and as a disinfectant for fruits and vegetables in some countries.
Industrial Importance
Permanganate titration (permanganometry) is a standard analytical method for determining iron content in ores, water, and environmental samples.
Properties
- Type
- Redox
- Reversible
- No
- Energy
- Exothermic
- ΔH
- -536.0 kJ/mol
Related Reactions
Aqua Regia Dissolving Gold
Bleaching with Sodium Hypochlorite
Cerium(IV) Reduction by Iron(II)
Chlorine Oxidation of Bromide
Chromate-Dichromate Equilibrium
Contact Process SO₂ Oxidation
Copper Displaced by Iron
Copper Oxidation by Nitric Acid
Copper Patina Formation (Verdigris)
Copper Reduction of Silver Ion
Frequently Asked Questions
What is the equation for Permanganate Oxidation of Iron(II)?
The balanced equation is: MnO₄⁻ + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O.
What type of reaction is Permanganate Oxidation of Iron(II)?
Permanganate Oxidation of Iron(II) is a redox reaction.
Is Permanganate Oxidation of Iron(II) exothermic or endothermic?
Permanganate Oxidation of Iron(II) is exothermic (releases energy). The enthalpy change (ΔH) is -536.0 kJ/mol.