Chlorine Oxidation of Bromide

Cl2 + 2Br− → 2Cl− + Br2

Übersicht

Chlorine oxidizes bromide ions to bromine while being reduced to chloride. This halogen displacement demonstrates the trend in oxidizing power: F₂ > Cl₂ > Br₂ > I₂. The reaction turns a colorless bromide solution orange-brown as molecular bromine is liberated.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Chlorine Cl 1 (g)
Produkt Bromine Br 1 (l)

Alltägliches Beispiel

Adding drops of chlorine water to a colorless bromide solution turns it orange-brown, a standard A-level chemistry experiment.

Industrielle Bedeutung

This reaction is the industrial method for extracting bromine from brine and seawater. Nearly all commercial bromine production uses chlorine displacement.

Eigenschaften

Typ
Redox
Reversibel
Nein
Energie
Exotherm
ΔH
-94,0 kJ/mol

Verwandte Reaktionen

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

Frequently Asked Questions

What is the equation for Chlorine Oxidation of Bromide?
The balanced equation is: Cl₂ + 2Br⁻ → 2Cl⁻ + Br₂.
What type of reaction is Chlorine Oxidation of Bromide?
Chlorine Oxidation of Bromide is a redox reaction.
Is Chlorine Oxidation of Bromide exothermic or endothermic?
Chlorine Oxidation of Bromide is exothermic (releases energy). The enthalpy change (ΔH) is -94.0 kJ/mol.