Iron Corrosion (Rusting)

4Fe + 3O2 + 6H2O → 4Fe(OH)3

概要

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).

参加者

役割 物質 係数 状態
反応物 Oxygen O 3 (g)
反応物 Iron Fe 4 (s)
反応物 Water H₂O 6 (l)

日常の例

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

産業上の重要性

腐食は世界経済に年間約2.5兆ドルのコストをもたらす。鉄の腐食の理解と防止は建設・製造・輸送インフラの維持に不可欠であり、防食コーティングや陰極防食技術の基盤となっている。

特性

タイプ
Redox
可逆的
いいえ
エネルギー
発熱性
ΔH
-1648.0 kJ/mol

関連する反応

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.