Arrange the following compounds in the increasing order of their boiling points

1. \(CH_3CH_2CH_2COOH\)
2. \(CH_3CH_2CH_2CH_2OH\)
3. \(CH_3CH_2OCH_2CH_3\)
4. \(CH_3CH_2CH_2CH_3\)
5. \(CH_3CH_2CH_2CHO\)

Choose the correct answer from the options given below:

D < B < A < E < C

The correct order of boiling points is:

D < B < A < E < C

This order can be determined by considering the intermolecular forces present in each compound.

Alkanes (D): Alkanes have only London dispersion forces, which are the weakest type of intermolecular force. As a result, alkanes have the lowest boiling points.

Branched Alkanes (B): Branched alkanes have slightly stronger London dispersion forces than straight-chain alkanes due to their more compact shape. As a result, branched alkanes have slightly higher boiling points than straight-chain alkanes of the same size.

Alcohols (C): Alcohols have hydrogen bonding in addition to London dispersion forces. Hydrogen bonding is a stronger intermolecular force than London dispersion forces. As a result, alcohols have higher boiling points than alkanes of the same size.

Aldehydes (E): Aldehydes have dipole-dipole interactions in addition to London dispersion forces. Dipole-dipole interactions are weaker than hydrogen bonding but stronger than London dispersion forces. As a result, aldehydes have higher boiling points than alkanes but lower boiling points than alcohols.

Carboxylic acids (A): Carboxylic acids have the strongest intermolecular forces due to hydrogen bonding. As a result, carboxylic acids have the highest boiling points.

Therefore, the correct order of boiling points is D < B < A < E < C.