Hydrolysis of Methyl Cyanide in the Presence of Acid

Methyl cyanide is a compound with the chemical formula CH3CN. Hydrolysis refers to the chemical reaction between a compound and water, which results in the splitting of a chemical bond and the formation of two new compounds. In the presence of acid, the hydrolysis of methyl cyanide gives ethanoic acid.

Explanation:

The hydrolysis of methyl cyanide in the presence of acid involves the following steps:

Step 1: Protonation of the Cyanide Group

The first step involves the protonation of the cyanide group in methyl cyanide by the acid. In the presence of an acid, the cyanide group accepts a proton (H+) and gets converted into a more reactive form called a protonated cyanide ion.

CH3CN + H+ → CH3C(NH)+

Step 2: Nucleophilic Attack by Water

In the second step, water acts as a nucleophile and attacks the protonated cyanide ion. The nucleophilic attack results in the formation of an intermediate compound called a hemiaminal.

CH3C(NH)OH

Step 3: Proton Transfer

In the third step, a proton transfer takes place from the hemiaminal to the acid, resulting in the formation of a carboxylic acid. The acid acts as a proton acceptor and accepts the proton from the hemiaminal. The end result is the formation of ethanoic acid.

CH3C(NH)OH + H+ → CH3COOH + NH+

Overall Reaction:

The overall reaction can be represented as follows:

CH3CN + H2O + H+ → CH3COOH + NH+

Conclusion:

In the presence of acid, the hydrolysis of methyl cyanide gives ethanoic acid as the end product. This reaction involves the protonation of the cyanide group, nucleophilic attack by water, and proton transfer to the acid.