Difference between revisions of "Combustion reactions"
(added links and words and category) |
Jazzman831 (talk | contribs) (merge with complete combustion reaction and incomplete combustion) |
||
| Line 1: | Line 1: | ||
| − | '''Combustion reactions''' are | + | '''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== | ||
Revision as of 03:06, July 23, 2007
Combustion reactions (informally known as simply burning) are chemical reactions in which a substance is reacted exothermically with molecular oxygen (O2) at a high temperature. Combustion reactions can either be complete or incomplete.[1]
In ideal circumstances, all reactions would be complete; or in other words, oxygen would fully oxidize the other reactants. For example, a combustion reaction involving a hydrocarbon (any molecule consisting only of carbon and hydrogen) would result in only carbon dioxide (CO2) and and water (H2O) 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.[1] 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.