Combustion+Reaction

Also called burning is the process of exothermic chemical reactions between a fuel and an oxidant followed by the production of heat and conversion of chemicals. The release of heat can result in the production of either glowing light or a flame. Said fuels often include organic compounds (hydrocarbons for example) in the gas liquid or solid phase.

2 H2 + O2 → 2 H2O(g) + heat is an example of the combustion of hydrogen and oxygen. This reaction is most commonly used for rocket engines.

COMPLETE AND INCOMPLETE COMBUSTION REACTIONS

COMPLETE-

In complete combustion, the reactant burns in oxygen, producing a limited number of products. When a hydrocarbon burns in oxygen, the reaction will only create carbon dioxide and water. When elements are burned, the products are primarily the most common oxides. Carbon will create carbon dioxide, nitrogen will create nitrogen dioxide, sulfur will create sulfur dioxide, and iron will create iron III oxide.

Below is a formula for combustion of methane in the air. CH4 + 2 O2 → CO2 + 2 H2O2 CH4 + 3 O2 → 2 CO + 4 H2O N2 + O2 → 2 NON2 + 2 O2 → 2 NO2

IMCOMPLETE

Incomplete combustion will only occur when there isn't enough oxygen to allow the fuel to react completely to produce carbon dioxide and water. It also happens when the combustion is doused by a heat sink such as a solid surface. For most fuels, such as diesel oil, coal or wood, decomposition of the organic material (Pyrolysis) occurs before combustion. In incomplete combustion, products of pyrolysis remain unburnt and contaminate the smoke with noxious particulate matter and gases. Partial oxidation of ethanol can produce harmful compounds for example carbon can produce toxic carbon monoxide.

To create a flame in a biome a peice of paper was dipped in menthol and relased CH 3 OH into the air.