Combustion is also currently the only reaction used to power rockets. The thermal energy produced from combustion of either fossil fuels such as coal or oil, or from renewable fuels such as firewood, is harvested for diverse uses such as cooking, production of electricity or industrial or domestic heating. Usually, the fuel is carbon, hydrocarbons, or more complicated mixtures such as wood that contains partially oxidized hydrocarbons. 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. Since burning is rarely clean, fuel gas cleaning or catalytic converters may be required by law.įires occur naturally, ignited by lightning strikes or by volcanic 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. ![]() Thus, the produced smoke is usually toxic and contains unburned or partially oxidized 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). Thermodynamically, the chemical equilibrium of combustion in air is overwhelmingly on the side of the products. Complete combustion is stoichiometric concerning the fuel, where there is no remaining fuel, and ideally, no residual oxidant. Uncatalyzed combustion in air requires relatively high temperatures. The heat of combustion is approximately −418 kJ per mole of O 2 used up in the combustion reaction, and can be estimated from the elemental composition of the fuel. 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 CH 4 is nearly the same as that of CO 2. This reaction releases 242 kJ/ mol of heat and reduces the enthalpy accordingly (at constant temperature and pressure):Ĭombustion of an organic fuel in air is always exothermic because the double bond in O 2 is much weaker than other double bonds or pairs of single bonds, and therefore the formation of the stronger bonds in the combustion products CO 2 and H 2O results in the release of energy. A simple example can be seen in the combustion of hydrogen and oxygen into water vapor, a reaction commonly used to fuel rocket engines. Combustion is often hot enough that incandescent light in the form of either glowing or a flame is produced. 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. While the activation energy must be overcome to initiate combustion (e.g., using a lit match to light a fire), the heat from a flame may provide enough energy to make the reaction self-sustaining.Ĭombustion is often a complicated sequence of elementary radical reactions. Combustion does not always result in fire, because a flame is only visible when substances undergoing combustion vapourise, but when it does, a flame is a characteristic indicator of the reaction. ![]() Air pollution abatement equipment provides combustion control for industrial processes.Ĭombustion, 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.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |