| Nitromethane |
| Systematic name|| nitromethane|
| Other names|| nitrocarbol|
| Molecular formula|| CH3NO2|
| SMILES || C[N+]([O-])=O|
| Molar mass|| 61.04 g/mol|
| Appearance||-|| CAS number|| [75-52-5]|
| Density and phase|| 1.138 g/cm3, liquid|
| Solubility in water|| miscible|
| Melting point|| -29 °C (244.15 K) |
| Boiling point|| 100-103 °C (373-376 K)|
| Acidity (pKa) || 10.2|
| Viscosity|| ? cP at ? °C |
| Hazards |
| MSDS|| External MSDS |
| Main hazards|| Flammable, harmful|
| NFPA 704|| |
| Flash point|| 35 °C|
| R/S statement|| R: R5 R10 R22 |
| RTECS number|| PA9800000|
| Related compounds|
| Related nitro compounds || nitroethane|
| Related compounds || methyl nitrite|
| Except where noted otherwise, data are given for|
materials in their standard state (at 25 °C, 100 kPa)
Infobox disclaimer and references
Nitromethane is an organic compound with the chemical formula CH3NO2. It is the simplest organic nitro compound. It is a slightly viscous, highly polar liquid commonly used as a solvent in a variety of industrial applications such as in extractions, as a reaction medium, and as a cleaning solvent. As an intermediate in organic synthesis, it is used widely in the manufacture of pharmaceuticals, pesticides, explosives, fibers, and coatings. It also finds use as a racing fuel.
Synthetic chemistry applications
Nitromethane is a popular solvent in organic and electroanalytical chemistry.
[Coetzee, J. F. and Chang, T. H., "Recommended Methods for the Purification of Solvents and Tests for Impurities: Nitromethane", Pure Appl. Chem., 1986, 58, 1541-1545.]
In organic synthesis nitromethane is employed as a one carbon building block. Its weak acidicity allows it to undergo deprotonation, enabling condensation reactions analogous to those of carbonyl compounds. Thus, under base catalysis, nitromethane adds to aldehydes in 1,2-addition in the nitroaldol reaction. Nitromethane can serve as a Michael donor, adding to α,β-unsaturated carbonyl compounds via 1,4-addition in the Michael reaction.
Use as an engine fuel
Nitromethane is used as a fuel in racing, particularly drag racing, to provide more power.
[K. Owen and T. Coley, "Automotive Fuels Reference Book - 2nd edition", Chapter 13 "Racing Fuels", ISBN 1-56091-589-7 (1995)] In this context, it is commonly referred to as "nitro" or "fuel".
The oxygen content of nitromethane enables it to burn with much less atmospheric oxygen in comparison to hydrocarbons such as gasoline:
- 4CH3NO2 + 3O2 → 4CO2 + 6H2O + 2N2
14.6 kg of air are required to burn one kg of gasoline, but only 1.7 kg of air for one kg of nitromethane. Since an engine’s cyliner can only contain a limited amount of air on each stroke, 8.7 times more nitromethane than gasoline can be burned in one stroke. However, nitromethane has a lower energy density. Gasoline provides about 42-44 MJ/kg, nitromethane provides only 11.3 MJ/kg. This analysis indicates that nitromethane generate about 2.3 times the power of gasoline.
Nitromethane can also be used as a monopropellant. Without additional oxygen nitromethane will combust according to:
- 4CH3NO2 → 4CO + 4H2O + 2H2 + 2N2
Nitromethane has a laminar combustion velocity of approx. 0.5 m/s, somewhat higher than gasoline. Thus nitromethane is suitable for high speed engines. Somewhat higher is also the flame temperature at about 2400 °C. The high heat of vaporisation of 0.56 MJ/kg together with the high fuel flow does however provide a high cooling of the incoming charge (about twice that of methanol), resulting in reasonably low temperatures. In a Top Fuel dragracing engine this alone will provide the cooling of the engine.
Nitromethane is usually used with rich air/fuel mixtures. This is partly because nitromethane can provide power even in the absence of atmospheric oxygen, as described above, but it's also because nitromethane tends to produce severe knock and pre-ignition. Rich mixtures do however cause ignition problems and a lower combustion speed.
When rich air/fuel mixtures are used, hydrogen and carbon monoxide will be two of the combustion products, when these and any unburned fuel comes into contact with the oxygen in the atmosphere at the end of the exhaust pipes they often ignite. The result is spectacular flames from the exhaust system.
A small amount of hydrazine blended in nitromethane can increase the power output even further. With nitromethane, hydrazine forms an explosive salt that can combust by using only the oxygen in the nitromethane. This mixture is however unstable, so it poses a severe safety hazard.
In addition, model aircraft and car fuel contains from 0% to 65% nitromethane. It has also been used as a model rocket fuel. It is normally mixed with methanol.
Nitromethane was not known to be an explosive until the 1950s, when a railroad tanker car of it exploded. Much testing later it was realized that nitromethane was a more energetic high explosive than TNT. However TNT has a higher velocity of detonation and brisance (shattering power against hard targets). Both of these explosives are oxygen poor and some benefits are gained from mixing with an oxidizer, such as ammonium nitrate. One graphic example of this was the use of nitromethane and ammonium nitrate on the Alfred P. Murrah Federal Building at Oklahoma City. Pure nitromethane is an insensitive explosive, but even so inhibitors may be used to reduce the hazards. The tank car explosion was speculated to be due to adiabatic compression, a hazard common to all liquid explosives. This is when small entrained air bubbles compress and superheat with rapid rises in pressure. It was thought that an operator rapidly snapped shut a valve creating a 'hammer-lock' pressure surge. Nitromethane can be sensitized by adding a base to raise the pH.