Chlorine Oxidation of Bromide

Cl2 + 2Br− → 2Cl− + Br2

Overview

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.

Participants

Role Substance Coefficient State
Reactant Chlorine Cl 1 (g)
Product Bromine Br 1 (l)

Everyday Example

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

Industrial Importance

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

Properties

Type
Redox
Reversible
No
Energy
Exothermic
ΔH
-94.0 kJ/mol

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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.