Combustion | Wikipedia audio article

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00:03:56 1 Types
00:04:05 1.1 Complete and incomplete
00:04:14 1.1.1 Complete
00:06:18 1.1.2 Incomplete
00:08:11 1.1.2.1 Incomplete combustion produced carbon monoxide
00:08:44 1.1.2.2 Problems associated with incomplete combustion
00:10:07 1.2 Smouldering
00:10:57 1.3 Rapid
00:11:37 1.4 Spontaneous
00:12:13 1.5 Turbulent
00:12:35 1.6 Micro-gravity
00:13:42 1.7 Micro-combustion
00:14:07 2 Chemical equations
00:14:17 2.1 Stoichiometric combustion of a hydrocarbon in oxygen
00:16:16 2.2 Stoichiometric combustion of a hydrocarbon in air
00:19:48 2.3 Trace combustion products
00:19:53 2.4 Incomplete combustion of a hydrocarbon in oxygen
00:21:26 3 Fuels
00:25:57 3.1 Liquid fuels
00:26:19 3.2 Gaseous fuels
00:26:54 3.3 Solid fuels
00:27:41 4 Combustion management
00:28:36 5 Reaction mechanism
00:30:57 5.1 Kinetic modelling
00:35:10 6 Temperature
00:35:31 7 Instabilities
00:37:33 8 See also
00:39:21 9 References



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SUMMARY
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Combustion, or burning, is a high-temperature exothermic redox chemical reaction between a fuel (the reductant) and an oxidant, usually atmospheric oxygen, that produces oxidized, often gaseous products, in a mixture termed as smoke. Combustion in a fire produces a flame, and the heat produced can make combustion self-sustaining. Combustion is often a complicated sequence of elementary radical reactions. Solid fuels, such as wood and coal, first undergo endothermic pyrolysis to produce gaseous fuels whose combustion then supplies the heat required to produce more of them. Combustion is often hot enough that incandescent light in the form of either glowing or a flame is produced. A simple example can be seen in the combustion of hydrogen and oxygen into water vapor, a reaction commonly used to fuel rocket engines. This reaction releases 242 kJ/mol of heat and reduces the enthalpy accordingly (at constant temperature and pressure):

2H2(g) + O2(g) → 2 H2O(g)Combustion of an organic fuel in air is always exothermic because the double bond in O2 is much weaker than other double bonds or pairs of single bonds, and therefore the formation of the stronger bonds in the combustion products CO2 and  H2O results in the release of energy. The bond energies in the fuel play only a minor role, since they are similar to those in the combustion products; e.g., the sum of the bond energies of CH4 is nearly the same as that of CO2. The heat of combustion is approximately -418 kJ per mole of O2 used up in the combustion reaction, and can be estimated from the elemental composition of the fuel.Uncatalyzed combustion in air requires fairly high temperatures. Complete combustion is stoichiometric with respect to the fuel, where there is no remaining fuel, and ideally, no remaining oxidant. Thermodynamically, the chemical equilibrium of combustion in air is overwhelmingly on the side of the products. However, complete combustion is almost impossible to achieve, since the chemical equilibrium is not necessarily reached, or may contain unburnt products such as carbon monoxide, hydrogen and even carbon (soot or ash). Thus, the produced smoke is usually toxic and contains unburned or partially oxidized products. Any combustion at high temperatures in atmospheric air, which is 78 percent nitrogen, will also create small amounts of several nitrogen oxides, commonly referred to as NOx, since the combustion of nitrogen is thermodynamically favored at high, but not low temperatures. Since combustion is rarely clean, flue gas cleaning or catalytic converters may be required by law.
Fires occur naturally, ignited by lightning strikes or by volcanic products. Combustion (fire) was the first controlled chemical reaction discovered by humans, in the form of campfires and bonfires, and continues to be the main method to produce energy for humanity. Usually, the fuel ...