Iron(II) to Iron(III) Oxidation by Oxygen

4Fe2+ + O2 + 4H+ → 4Fe3+ + 2H2O

Übersicht

Ferrous ions (Fe²⁺) are oxidized to ferric ions (Fe³⁺) by dissolved oxygen in acidic solution. This reaction is responsible for the yellowing of iron-containing groundwater upon exposure to air. The green Fe²⁺ solution turns yellow-brown as Fe³⁺ forms.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Oxygen O 1 (g)
Produkt Water H₂O 2 (l)

Alltägliches Beispiel

Well water that is clear underground but turns rusty brown when left standing is undergoing this oxidation of dissolved iron(II) by air.

Industrielle Bedeutung

Iron(II)/iron(III) redox chemistry is fundamental to water treatment, geochemistry, soil science, and corrosion engineering.

Eigenschaften

Typ
Redox
Reversibel
Nein
Energie
Exotherm
ΔH
-176,0 kJ/mol

Verwandte Reaktionen

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) Zinc Reduction of Silver Ion Displacement of Hydrogen from Acid by Magnesium

Frequently Asked Questions

What is the equation for Iron(II) to Iron(III) Oxidation by Oxygen?
The balanced equation is: 4Fe²⁺ + O₂ + 4H⁺ → 4Fe³⁺ + 2H₂O.
What type of reaction is Iron(II) to Iron(III) Oxidation by Oxygen?
Iron(II) to Iron(III) Oxidation by Oxygen is a redox reaction.
Is Iron(II) to Iron(III) Oxidation by Oxygen exothermic or endothermic?
Iron(II) to Iron(III) Oxidation by Oxygen is exothermic (releases energy). The enthalpy change (ΔH) is -176.0 kJ/mol.