What is Acetonitrile C2H3N?
Acetonitrile, often known as nitrile, is a methylated form of hydrogen cyanide (-CH3). Acetonitrile is a volatile organic molecule. Also known as Cyanomethane and Methanecarbonitrile. C2H3N is the chemical formula for acetonitrile. Methyl cyanide, sometimes known as acetonitrile, is a chemical compound having the formula CH3CN. It is mostly created as a byproduct of acrylonitrile production. It is employed in chemical synthesis and the purification of butadiene as a polar aprotic solvent.
Cyanomethane is a colourless, odourless liquid with no discernible hue. It has a flash point of 420 F and is less dense than water. Its vapours have a greater density than air. The flavour of methanecarbonitrile is sweet and scorching, and it is readily soluble in water.
Structure of Acetonitrile CH3CN
Properties of Acetonitrile – C2H3N
| Acetonitrile | C2H3N |
| Molecular Weight of Acetonitrile | 41.053 g/mol |
| Density of Acetonitrile | 0.786 g/cm3 |
| Melting Point of Acetonitrile | −46 to −44 °C |
| Boiling point of Acetonitrile | 81.3 to 82.1 °C |
Chemical Properties of Acetonitrile (C2H3N)
Reaction with Concentrated HCl
Acetamide is the result of the partial hydrolysis of acetonitrile in cold-concentrated HCl. On complete hydrolysis, carboxylic acid is produced.
Reaction with phenyl magnesium bromide
Nitriles combine with the Grignard reagent to produce ketones. Nitriles, represented by the formula RC≡N, react with Grignard reagents or organolithium reagents to form ketones. Similar to aldehydes and ketones, organometallic reagents with a strong nucleophilicity contribute to the C≡N bond.
Acetonitrile Molecular Formula
CH3CN or C2H3N
Preparation of Acetonitrile
It is a byproduct of the production of acrylonitrile. It can also be produced through the hydrogenation of ammonia and carbon monoxide mixtures or the dehydration of acetamide.
Health Hazards
This substance is harmful when absorbed via the skin. It is extremely combustible and emits hazardous vapours or fumes when ignited. Cyanomethane air or vapour combinations are explosive. When it comes into contact with a powerful oxidising agent, it can explode. When heated, it might rupture due to an increase in pressure.
Severe exposures can produce skin eruptions, delirium, paralysis, irritability, confusion, and convulsions.
Despite its toxicity, it has been utilised in recipes for nail polish removal. At least two incidences of accidental poisoning of young children by nail polish remover containing acetonitrile have been documented, one of which was deadly.
Since March 2000, the European Economic Area has prohibited the use of acetonitrile in cosmetics. Acetone and ethyl acetate are often favoured as safer alternatives for home use.
Uses of Acetonitrile (C2H3N)
- As a solvent, acetonitrile is used in the extraction of hydrocarbons.
- It is used to extract vegetable oil from fatty acids.
- Used to create perfumes.
- It is commonly employed in the synthesis of medicines.
- It is utilised in the production of rubber.
- It is utilised in the refining and extraction of copper.
- Used in electrochemical cells as a solvent.
Frequently Asked Questions – FAQs
Q.1 What is acetonitrile used for?
Pharmaceuticals, perfumes, rubber goods, insecticides, batteries, and acrylic nail removers are produced using acetonitrile. Additionally, this is utilised to extract fatty acids from vegetable and animal oils.
Q.2 Is acetonitrile more polar than methanol?
Methanol is a polar-protic solvent, whereas acetonitrile is a polar-aprotic solvent with a greater dipole moment.
Q.3 Is acetonitrile a powerful acid?
Acetonitrile, a common solvent in organic synthesis, can be hydrolyzed in the presence of a strong aqueous base, such as NaOH or KOH, leading to a runaway reaction.
Q.4 Are acetone and acetonitrile the same?
Both acetonitrile and acetone are organic molecules, however, their chemical structures and physical and chemical properties vary. The molecule acetonitrile is a nitrile, whereas acetone is a ketone.
Q.5 How much acetonitrile is toxic?
The new IDLH for acetonitrile is 500 ppm, as determined by acute inhalation toxicity studies in humans [Deichmann and Gerard 1969]. Due to the lack of acute toxicity data for employees exposed to concentrations beyond 500 ppm, this figure may be cautious.
