Iron Corrosion (Rusting)

4Fe + 3O2 + 6H2O → 4Fe(OH)3

概述

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).

参与者

角色 物质 系数 状态
反应物 Oxygen O 3 (g)
反应物 Iron Fe 4 (s)
反应物 Water H₂O 6 (l)

日常示例

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

工业重要性

腐蚀每年给全球经济造成超过2.5万亿美元的损失，约占GDP的3.4%。防腐技术（热镀锌、阴极保护、涂层）对基础设施、交通运输和制造业至关重要。

属性

类型
Redox
可逆
否
能量
放热
ΔH
-1648.0 kJ/mol

相关反应

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.