Specification :

CAS No.: 75-52-5
EINECS: 200-876-6
HS code: 2904909090
Molecular Formula: CH3NO2
Molecular Weight61.04

Specification:
Density: 1.1371
Melting point: -29 ºC
Boiling point: 100-102 ºC
Refractive index: 1.3805-1.3825
Flash point: 35 ºC
Water solubility: 9.5 g/100 mL (20 ºC)

Preparation:
Nitromethane is produced industrially by treating propane with nitric acid at 350–450 °C. This exothermic reaction produces the four industrially significant nitroalkanes: nitromethane, nitroethane, 1-nitropropane, and 2-nitropropane. The reaction involves free radicals, including the alkoxyl radicals of the type CH3CH2CH2O., which arise via homolysis of the corresponding nitrite ester. These alkoxy radicals are susceptible to C-C fragmentation reactions, which explains the formation of a mixture of products.[1]
Although inexpensively available, nitromethane can be prepared in other methods that are of instructional value. The reaction of sodium chloroacetate with sodium nitrite in aqueous solution produces this compound:
ClCH2COONa + NaNO2 + H2O ’ CH3NO2 + NaCl + NaHCO3

Usage:
The principal use of nitromethane is as a stabilizer for chlorinated solvents, which are used in dry cleaning, semiconductor processing, and degreasing. It is also used most effectively as a solvent or dissolving agent for acrylate monomers, such as cyanoacrylates (more commonly known as "super-glue").

Purification:
Nitromethane is a popular solvent in organic and electroanalytical chemistry. It can be purified by cooling below its freezing point, washing the solid with cold diethyl ether, followed by distillation.

Safety Protection:
Harmful; Heating may cause an explosion; Flammable; Harmful if swallowed. In case of fire and / or explosion do not breathe fumes.

Derivatives:
In organic synthesis nitromethane is employed as a one carbon building block. Its 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. Some important derivatives include the pesticides Chloropicrin, Cl3CNO2 and tris(hydroxymethyl)nitromethane, (HOCH2)3CNO2. Reduction of the latter gives tris(hydroxymethyl)aminomethane, (CH2OH)3CNH2, better known as “tris,� a widely used buffer.
In more specialized organic synthesis, nitromethane serves as a Michael donor, adding to ±,²-unsaturated carbonyl compounds via 1,4-addition in the Michael reaction.

As an engine fuel:
In a minor application, nitromethane is used as a fuel in racing, particularly drag racing, as well as for rockets and model airplanes and commonly referred to in this context as "nitro". 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 is required to burn one kilogram of gasoline, but only 1.7 kg of air for one kilogram of nitromethane. Since an engine’s cylinder can only contain a limited amount of air on each stroke, 8.7 times more nitromethane than gasoline can be burned in one stroke. Nitromethane, however, has a lower energy density: Gasoline provides about 42–44 MJ/kg whereas nitromethane provides only 11.3 MJ/kg. This analysis indicates that nitromethane generates about 2.3 times the power of gasoline when combined with a given amount of oxygen.
Nitromethane can also be used as a monopropellant, i.e., a fuel that burns without added oxygen. The following equation describes this process:
4 CH3NO2 ’ 4 CO + 4 H2O + 2 H2 + 2 N2
Nitromethane has a laminar combustion velocity of approx. 0.5 m/s, somewhat higher than gasoline, thus making it suitable for high speed engines. It also has a somewhat higher flame temperature of about 2400 °C. The high heat of vaporisation of 0.56 MJ/kg together with the high fuel flow provides significant cooling of the incoming charge (about twice that of methanol), resulting in reasonably low temperatures.
Nitromethane is usually used with rich air/fuel mixtures because it provides power even in the absence of atmospheric oxygen. When rich air/fuel mixtures are used, hydrogen and carbon monoxide are two of the combustion products. These gases often ignite, sometimes spectacularly, as the normally very rich mixtures of the still burning fuel exits the exhaust ports. Very rich mixtures are necessary to reduce the temperature of combustion chamber hot parts in order to control pre-ignition and subsequent detonation. Operational details depend on the particular mixture and engine characteristics.
A small amount of hydrazine blended in nitromethane can increase the power output even further. With nitromethane, hydrazine forms an explosive salt that is again a monopropellant. This unstable mixture poses a severe safety hazard.
In model aircraft and car glow fuel, the primary ingredient is generally methanol with some nitromethane (0% to 65%, but rarely over 30% since nitromethane is expensive compared to methanol) and 10–20% lubricants (usually castor oil and/or synthetic oil). Even moderate amounts of nitromethane tend to increase the power created by the engine (as the limiting factor is often the air intake), making the engine easier to tune (adjust for the proper air/fuel ratio).

Explosive properties:
Nitromethane was not known to be a high explosive until a railroad tanker car loaded with it exploded on June 1, 1958.[2] After much testing it was realized that nitromethane was a more energetic high explosive than TNT, although TNT has a higher velocity of detonation and brisance. Both of these explosives are oxygen poor and some benefits are gained from mixing with an oxidizer, such as ammonium nitrate. Pure nitromethane is an insensitive explosive with a VoD of approximately 6200 m/s, 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.
Nitromethane can also be mixed with ammonium nitrate, which is used as an oxidizer, to form an explosive mixture known as ANNM. One graphic example of this was the use of nitromethane and ammonium nitrate on the Alfred P. Murrah Federal Building at Oklahoma City.