Combustion of Butane

2C4H10 + 13O2 → 8CO2 + 10H2O

Übersicht

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.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Butane C₄H₁₀ 2 (g)
Reaktant Oxygen O 13 (g)
Produkt Carbon Dioxide CO₂ 8 (g)
Produkt Water H₂O 10 (l)

Alltägliches Beispiel

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

Industrielle Bedeutung

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

Eigenschaften

Typ
Combustion
Reversibel
Nein
Energie
Exotherm
ΔH
-5754,0 kJ/mol

Verwandte Reaktionen

Combustion of Carbon Monoxide Combustion of Ethylene Combustion of Glycerol Combustion of Methanol Combustion of Phenol Combustion of Naphthalene Combustion of Methane Combustion of Octane (Gasoline) Combustion of Hydrogen Gas Combustion of Benzene

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.