Hydrogen Peroxide Disproportionation

2H2O2 → 2H2O + O2

Visão geral

Hydrogen peroxide simultaneously acts as both oxidizing and reducing agent in this disproportionation reaction. One molecule is reduced to water (O goes from -1 to -2) while another is oxidized to oxygen gas (O goes from -1 to 0). Manganese dioxide or the enzyme catalase dramatically accelerate this reaction.

Participantes

Papel Substância Coeficiente Estado
Reagente Hydrogen Peroxide H₂O₂ 2 (aq)
Produto Oxygen O 1 (g)
Produto Water H₂O 2 (l)

Exemplo do cotidiano

The fizzing when hydrogen peroxide is applied to a wound occurs because catalase enzyme in blood rapidly decomposes H₂O₂, releasing oxygen bubbles.

Importância industrial

A decomposição de H₂O₂ é utilizada no tratamento de águas residuais, como propulsor (H₂O₂ concentrado em torpedos e naves espaciais) e na geração de oxigénio. A catalase está presente em quase todos os organismos como proteção contra o stress oxidativo.

Propriedades

Tipo
Redox
Reversível
Não
Energia
Exotérmico
ΔH
-196,1 kJ/mol
Catalisador
MnO₂ or catalase enzyme

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Frequently Asked Questions

What is the equation for Hydrogen Peroxide Disproportionation?
The balanced equation is: 2H₂O₂ → 2H₂O + O₂.
What type of reaction is Hydrogen Peroxide Disproportionation?
Hydrogen Peroxide Disproportionation is a redox reaction.
Is Hydrogen Peroxide Disproportionation exothermic or endothermic?
Hydrogen Peroxide Disproportionation is exothermic (releases energy). The enthalpy change (ΔH) is -196.1 kJ/mol.
What conditions are needed for Hydrogen Peroxide Disproportionation?
This reaction requires a catalyst (MnO₂ or catalase enzyme).