Halogenation of Methane (Chlorination)

CH₄ + Cl₂ → CH₃Cl + HCl

Overview

Methane undergoes free radical substitution with chlorine in the presence of UV light or heat. The mechanism involves initiation (Cl₂ → 2Cl·), propagation (Cl· + CH₄ → CH₃· + HCl, CH₃· + Cl₂ → CH₃Cl + Cl·), and termination. Further substitution can produce CH₂Cl₂, CHCl₃, and CCl₄.

Participants

Role	Substance	Coefficient	State
Reactant	Methane CH₄	1	(g)
Reactant	Chlorine Cl	1	(g)
Product	Hydrochloric Acid HCl	1	(g)

Everyday Example

Chloroform (CHCl₃), historically used as an anesthetic, is produced by multiple chlorination of methane.

Industrial Importance

Chloromethane (CH₃Cl) is used as a methylating agent and refrigerant. Dichloromethane is a widely used solvent. Chloroform is an important chemical intermediate.

Properties

Type: Organic
Reversible: No
Energy: Exothermic
ΔH: -98.0 kJ/mol
Catalyst: UV light or heat

Related Reactions

Aldol Condensation of Acetaldehyde Amide Formation (Acetic Acid + Ammonia) Baeyer-Villiger Oxidation Beckmann Rearrangement (Cyclohexanone Oxime) Bromination of Ethylene Buchwald-Hartwig Amination Cannizzaro Reaction of Formaldehyde Catalytic Hydrogenation of Ethylene Claisen Condensation (Ethyl Acetate) Condensation Polymerization (Nylon 6,6)

Frequently Asked Questions

What is the equation for Halogenation of Methane (Chlorination)?

The balanced equation is: CH₄ + Cl₂ → CH₃Cl + HCl.

What type of reaction is Halogenation of Methane (Chlorination)?

Halogenation of Methane (Chlorination) is a organic reaction.

Is Halogenation of Methane (Chlorination) exothermic or endothermic?

Halogenation of Methane (Chlorination) is exothermic (releases energy). The enthalpy change (ΔH) is -98.0 kJ/mol.

What conditions are needed for Halogenation of Methane (Chlorination)?

This reaction requires a catalyst (UV light or heat).