Permanganate Oxidation of Oxalic Acid

2MnO4− + 5C2O42− + 16H+ → 2Mn2+ + 10CO2 + 8H2O

Visão geral

Permanganate oxidizes oxalate to CO₂ while Mn(VII) is reduced to Mn(II). This reaction is autocatalytic: the Mn²⁺ product catalyzes the reaction, so it starts slowly and accelerates dramatically. The purple permanganate is decolorized as the reaction proceeds. It is a classic redox titration used in analytical chemistry.

Participantes

Papel Substância Coeficiente Estado
Reagente Oxalic Acid C₂H₂O₄ 5 (aq)
Produto Water H₂O 8 (l)
Produto Carbon Dioxide CO₂ 10 (g)

Exemplo do cotidiano

This reaction demonstrates autocatalysis: the first drops of permanganate decolorize slowly, but later drops disappear almost instantly.

Importância industrial

A titulação permanganato-oxalato é utilizada para padronizar soluções de permanganato e como exemplo didático de cinética autocatalítica.

Propriedades

Tipo
Redox
Reversível
Não
Energia
Exotérmico
ΔH
-489,0 kJ/mol

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Frequently Asked Questions

What is the equation for Permanganate Oxidation of Oxalic Acid?
The balanced equation is: 2MnO₄⁻ + 5C₂O₄²⁻ + 16H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O.
What type of reaction is Permanganate Oxidation of Oxalic Acid?
Permanganate Oxidation of Oxalic Acid is a redox reaction.
Is Permanganate Oxidation of Oxalic Acid exothermic or endothermic?
Permanganate Oxidation of Oxalic Acid is exothermic (releases energy). The enthalpy change (ΔH) is -489.0 kJ/mol.