Iron Corrosion (Rusting)

4Fe + 3O2 + 6H2O → 4Fe(OH)3

개요

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).

참여 물질

역할 물질 계수 상태
반응물 Oxygen O 3 (g)
반응물 Iron Fe 4 (s)
반응물 Water H₂O 6 (l)

일상 속 예시

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

산업적 중요성

전 세계 철강 손실의 주요 원인으로, 방식 코팅(도장, 아연 도금), 음극 방식, 내식성 합금 개발 산업을 이끕니다. 건축, 교량, 선박, 자동차 내구성에 직접적 영향을 미칩니다.

성질

유형
Redox
가역 반응
아니오
에너지
발열
ΔH
-1648.0 kJ/mol

관련 반응

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.