Combustion of Butane

2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O

Overview

Butane burns in oxygen to produce carbon dioxide and water. Butane is the primary fuel in disposable cigarette lighters and portable camping stoves. It has a higher energy density than propane but requires more oxygen for complete combustion.

Participants

Role	Substance	Coefficient	State
Reactant	Butane C₄H₁₀	2	(g)
Reactant	Oxygen O	13	(g)
Product	Carbon Dioxide CO₂	8	(g)
Product	Water H₂O	10	(l)

Everyday Example

Every time you flick a disposable lighter, you are initiating butane combustion. Butane also powers portable camping stoves.

Industrial Importance

Butane is a component of LPG, used as a fuel, refrigerant, and chemical feedstock for butadiene and maleic anhydride production.

Properties

Type: Combustion
Reversible: No
Energy: Exothermic
ΔH: -5754.0 kJ/mol

Related Reactions

Combustion of Acetylene Combustion of Benzene Combustion of Carbon Monoxide Combustion of Cyclohexane Combustion of Ethane Combustion of Ethanol Combustion of Ethylene Combustion of Glucose (Cellular Respiration) Combustion of Glycerol Combustion of Hexane

Frequently Asked Questions

What is the equation for Combustion of Butane?

The balanced equation is: 2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O.

What type of reaction is Combustion of Butane?

Combustion of Butane is a combustion reaction.

Is Combustion of Butane exothermic or endothermic?

Combustion of Butane is exothermic (releases energy). The enthalpy change (ΔH) is -5754.0 kJ/mol.