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All alkanes react with oxygen in a combustion reaction, although they become increasingly difficult to ignite as the number of carbon atoms increases. The general equation for complete combustion is: C n H 2n+2 + ( 3 / 2 n + 1 / 2 ) O 2 → (n + 1) H 2 O + n CO 2 or C n H 2n+2 + ( 3n + 1 / 2 ) O 2 → (n + 1) H 2 O + n CO 2
Nonane undergoes combustion reactions that are similar to other alkanes. In the presence of sufficient oxygen, nonane burns to form water and carbon dioxide. C 9 H 20 + 14O 2 → 9CO 2 + 10H 2 O. When insufficient oxygen is available for complete combustion, the burning products include carbon monoxide. 2C 9 H 20 + 19O 2 → 18CO + 20H 2 O
A complete set of equations for the combustion of a hydrocarbon in the air, therefore, requires an additional calculation for the distribution of oxygen between the carbon and hydrogen in the fuel. The amount of air required for complete combustion is known as the "theoretical air" or "stoichiometric air". [3]
The combustion of a stoichiometric mixture of fuel and oxidizer (e.g. two moles of hydrogen and one mole of oxygen) in a steel container at 25 °C (77 °F) is initiated by an ignition device and the reactions allowed to complete. When hydrogen and oxygen react during combustion, water vapor is produced.
Decane is an alkane hydrocarbon with the chemical formula C 10 H 22. Although 75 structural isomers are possible for decane, the term usually refers to the normal-decane ("n-decane"), with the formula CH 3 (CH 2) 8 CH 3. All isomers, however, exhibit similar properties and little attention is paid to the composition. [5] These isomers are ...
2-Methyloctane burns in the same way as other alkanes. Where there is enough oxygen, nonane burns to form water and carbon dioxide, so 2-methyloctane would do the same. C 9 H 20 + 14 O 2 → 9 CO 2 + 10 H 2 O. When insufficient oxygen is present for complete combustion, carbon monoxide is produced. 2 C 9 H 20 + 19 O 2 → 18 CO + 20 H 2 O
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The constant volume adiabatic flame temperature is the temperature that results from a complete combustion process that occurs without any work, heat transfer or changes in kinetic or potential energy. Its temperature is higher than in the constant pressure process because no energy is utilized to change the volume of the system (i.e., generate ...