Iron Corrosion (Rusting)

4Fe + 3O2 + 6H2O → 4Fe(OH)3

Übersicht

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).

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Oxygen O 3 (g)
Reaktant Iron Fe 4 (s)
Reaktant Water H₂O 6 (l)

Alltägliches Beispiel

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

Industrielle Bedeutung

Corrosion costs the global economy over $2.5 trillion annually. Understanding and preventing iron corrosion is critical for infrastructure, transportation, and manufacturing.

Eigenschaften

Typ
Redox
Reversibel
Nein
Energie
Exotherm
ΔH
-1648,0 kJ/mol

Verwandte Reaktionen

Iron(II) to Iron(III) Oxidation by Oxygen Bleaching with Sodium Hypochlorite Copper Reduction of Silver Ion Aqua Regia Dissolving Gold Cerium(IV) Reduction by Iron(II) Copper Oxidation by Nitric Acid Hypochlorite Oxidation of Hydrogen Peroxide Hydrogen Peroxide as Oxidizing Agent (Acidic) Hydrogen Peroxide Disproportionation Displacement of Hydrogen from Acid by Magnesium

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.