Iron Corrosion (Rusting)

4Fe + 3O2 + 6H2O → 4Fe(OH)3

Descripción general

Iron corrosion is an electrochemical process where iron is oxidized to Fe²⁺/Fe³⁺ at anodic sites while oxygen is reduced at cathodic sites. The process requires both water and oxygen. The initial Fe(OH)₂ product is further oxidized to Fe(OH)₃, which dehydrates to form rust (Fe₂O₃·nH₂O).

Participantes

Rol Sustancia Coeficiente Estado
Reactivo Oxygen O 3 (g)
Reactivo Iron Fe 4 (s)
Reactivo Water H₂O 6 (l)

Ejemplo cotidiano

A car's body rusting over time, iron nails turning orange-brown, and bridge structures corroding all involve this electrochemical process.

Importancia industrial

La corrosión cuesta a la economía mundial más de 2,5 billones de dólares anuales. Comprender y prevenir la corrosión del hierro es fundamental para la ingeniería civil, naval y de infraestructuras.

Propiedades

Tipo
Redox
Reversible
No
Energía
Exotérmico
ΔH
-1648,0 kJ/mol

Reacciones relacionadas

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Frequently Asked Questions

What is the equation for Iron Corrosion (Rusting)?
The balanced equation is: 4Fe + 3O₂ + 6H₂O → 4Fe(OH)₃.
What type of reaction is Iron Corrosion (Rusting)?
Iron Corrosion (Rusting) is a redox reaction.
Is Iron Corrosion (Rusting) exothermic or endothermic?
Iron Corrosion (Rusting) is exothermic (releases energy). The enthalpy change (ΔH) is -1648.0 kJ/mol.