Hydrogen Peroxide Disproportionation

2H2O2 → 2H2O + O2

Descripción general

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

Rol Sustancia Coeficiente Estado
Reactivo Hydrogen Peroxide H₂O₂ 2 (aq)
Producto Oxygen O 1 (g)
Producto Water H₂O 2 (l)

Ejemplo cotidiano

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

Importancia industrial

La descomposición del H₂O₂ se usa en el tratamiento de aguas residuales, como propelente concentrado y la actividad de la catalasa es importante en biotecnología y diagnóstico médico.

Propiedades

Tipo
Redox
Reversible
No
Energía
Exotérmico
ΔH
-196,1 kJ/mol
Catalizador
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).