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Acetamide or acetic acid or ethanamide is an inorganic compound. Furthermore, the simplest amide derived from acetic acid that’s why it is slightly acidic in nature. Some of its uses are an industrial solvent and plasticizers. Moreover, on a pH scale then it has a higher pH reading than acetone.
Acetamide Formula and Structure
The chemical formula of acetamide is C2H5NO or CH3CONH2. Moreover, its molar mass is 59.07 g/mol. The acetamide has a methyl group (-CH3) bound to a carbonyl (CO) and Amine (NH2). Besides, the acetamide primarily comprises of carboxylic acid amide functional group that has a general structure RC (=O) NH2.
Acetamide Formula Structure
Acetamide Occurrence
Generally, the acetamide occurs in burning waste coal piles that form between 50 and 150oC (122-302oF). Also, it only appears in periods of dry weather. Furthermore, the scientist has detected its presence near the center of the Milky Way galaxy.
Also, this finding is potentially significant for amino acids in proteins. Moreover, this finding lends support to the theory that organic molecules that can lend to life can form in space.
Production of Acetamide
An excellent amount of acetamide produced through ammonolysis of acetylacetone under conditions commonly used in reductive amination.
Besides, anhydrous acetic acid is also used to produce it, acetonitrile and very well dried hydrogen chloride gas, using an ice bath, together with more valuable reagent acetyl chloride. Typically, this product is low (up to 35 percent), and the acetamide produced in this way is generated as a salt with HCl.
However, on the industrial scale, they use a similar method that scientists use. In industries, they produce acetamide by dehydrating ammonium acetate or via the hydration of acetonitrile a by-product of the production of acrylonitrile.
CH3CN + H2O → CH3C(O)NH2
Physical Properties of Acetamide
| Chemical formula | C2H5NO |
| Molecular weight | 59.068 g/mol |
| Density | 1.159 g/cm3 |
| Melting point | 79 to 81 °C |
| Boiling point | 221.2 °C |
We can identify it in the field as transparent to translucent, colorless or gray variations. Also, it has a white streak. The density of acetamide is 1.17 g/cm3 and hardness of 1 to 1.5 roughly close to talc or a slightly harder substance. The melting point of acetamide is between 79 to 81oC, whereas its boiling point is 221.2oC.
Furthermore, its density is 1.159 g/cm3. Besides, it is soluble in water (2000 g L-1), ethanol (500 g L-1), pyridine (166.67 g L-1), chloroform, glycerol, hot benzene, slightly soluble in ether.
Chemical Properties of Acetamide
We find it as hygroscopic solid that is colorless and has a mousy odor which depends on its purity. Also, it has a bitter taste. Furthermore, it is a member of the class of acetamides which results from the formal condensation of acetic acid (CH3COOH) with ammonia (NH3). Most importantly, the carbonyl, methyl and anime groups share electrons with each other to form acetamide.
Acetamide Uses
Mainly, it is used as a solvent for many inorganic and organic compounds and in explosives. Furthermore, industries use it as a plasticizer and hygroscopic agent. Also, they use it to manufacture methylamine and as a stabilizer. Besides, it can act as a penetrating agent and fire suppressant.
Health and safety hazard
It has low toxicity which causes a reduction in weight which only happens when exposed to a high oral dose. Also, it mildly irritates mucous membranes, eyes, and skin. Furthermore, its combustion generates toxic gases or fumes. It can cause damage to corneal. Repeated oral exposure over time can cause liver tumors and lymphoma.
Uses of Acetamide-CH3CONH2
- Acetamide is used as a solvent for many inorganic and organic compounds.
- Used in explosives.
- Used as a plasticizer.
- Used as a hygroscopic agent.
- Used to manufacture methylamine.
- Used as a stabilizer.
- Used as a penetrating agent.
- Used as a fire suppressant.
Solved Example For You
Question: How scientists produce acetamide in laboratories?
Solution
In laboratories, scientists produce acetamide by hydration of ammonium acetate in this way.
[NH4][CH3CO2] → CH3C(O)NH2 + H2O
What is Acetamide?
C2H5NO is an organic compound with chemical name Acetamide.
Acetamide is also called Acetic acid amide, or Ethanamide or Acetimidic acid. It is derived from acetic acid and is the simplest amide. It is widely used as a plasticizer.
Ethanamide is obtained as a hygroscopic solid which is colourless and has a mousy odour. It is readily soluble in water, chloroform, hot benzene, glycerol and slightly soluble in ether. It is a member of the class of acetamides which results from the formal condensation of acetic acid (CH3COOH) with ammonia (NH3). It is naturally found in red beetroot.
Frequently Asked Questions
Q1
What is acetamide used for?
Acetamide is an organic compound that has the CH3CONH2 formula. This is the simplest amide of acetic acid derivatives. Acetamide is used in the manufacture of polymeric products, such as polyvinyl acetamide, a polymeric commodity used as an absorbent, as a co-monomer.
Q2
Why is acetamide soluble in water?
The primary amide is formed from NH2, amino group replacing the carboxylic hydroxyl group. A case in point is acetamide (acetic acid + amide). Low molecular weight amides caused by the formation of hydrogen bonds are soluble in water.
Q3
What does acetamide smell like?
Acetamide is an acetic acid-derived chemical that has been identified as smelling like vinegar or ammonia. It will cling to places where the musculus is sleeping and going to get food scrounge.
Q4
Is acetamide soluble in HCl?
The key findings have been that ammonia and acetamide are water and HCl soluble since they are smaller molecules. The compounds triethylamine, aniline, and N, N-dimethylaniline are not known to be water- and HCl soluble, but are MTBE-soluble. MTBE is not soluble in ammonia and acetamide.
Q5
Why is acetamide a weaker base than ethylamine?
The presence of a lone pair of electrons on a base determines its intensity as these electrons are the ones that will “mop up” H+ ions in solution and thus increase pH toward more alkaline conditions. Phenylamine is also a weaker base than ethylamine since there is less of a lone pair.
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