Iron Corrosion (Rusting)

4Fe + 3O2 + 6H2O → 4Fe(OH)3

نظرة عامة

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).

المشاركون

الدور المادة المعامل الحالة
متفاعل Oxygen O 3 (g)
متفاعل Iron Fe 4 (s)
متفاعل Water H₂O 6 (l)

مثال من الحياة اليومية

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

الأهمية الصناعية

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

الخصائص

النوع
Redox
قابل للعكس
لا
الطاقة
طارد للحرارة
ΔH
-1648,0 kJ/mol

التفاعلات ذات الصلة

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) Chlorine Oxidation of Bromide Copper Oxidation by Nitric Acid Hypochlorite Oxidation of Hydrogen Peroxide Hydrogen Peroxide as Oxidizing Agent (Acidic) 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.