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Line 1: − + − Incomplete combustion, typically resulting from a poor oxygen supply, also results in the formation of [[carbon monoxide]] (CO).+ − The [[carbon]] and [[hydrogen]] in the process come from the breakdown of the combusting material itself, while the oxygen typically comes from the environment.+ − − Combustion is usually [[exothermic]], that is, it liberates more [[energy]] than the [[reaction]] uses.
merge with complete combustion reaction and incomplete combustion
'''Combustion reactions''' are those in which [[oxygen]] (O<sub>2</sub>) is added while [[carbon dioxide]] (CO<sub>2</sub>) and [[water]] (H<sub>2</sub>0) are produced.<ref>Wile, Dr. Jay L. ''Exploring Creation With Chemistry''. Apologia Educational Ministries, Inc. 1998</ref>
'''Combustion reactions''' (informally known as simply ''burning'') are chemical reactions in which a substance is reacted [[exothermic]]ally with molecular [[oxygen]] (O<sub>2</sub>) at a high temperature. Combustion reactions can either be ''complete'' or ''incomplete''.<ref name="ref1">What is combustion? [http://www.habmigern2003.info/1_combustion.html]</ref>
In ideal circumstances, all reactions would be complete; or in other words, oxygen would fully [[oxidize]] the other [[reactant]]s. For example, a combustion reaction involving a [[hydrocarbon]] (any molecule consisting only of carbon and hydrogen) would result in only carbon dioxide (CO<sub>2</sub>) and and water (H<sub>2</sub>O) as products (possibly with excess oxygen).
In the real world, however, combustion reactions rarely go to completion. This is due to imperfect conditions, such as insufficient oxygen or low ignition temperature.<ref name="ref1" /> Incomplete combustion results in additional products which are not fully oxidized. For example, an incomplete combustion reaction involving a hydrocarbon would include [[carbon monoxide]] (CO) as a product, along with carbon dioxide and water.
==References==
==References==