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 < E < C < B < A

The correct answer is option 1. D < E < C < B < A.

Here is an explanation of why option 1 (D < E < C < B < A) is the correct order of boiling points for the compounds:

D: \(CH_3CH_2CH_2CH_3\) (Butane) 

Butane is a non-polar alkane. The only forces acting between its molecules are London dispersion forces (a type of van der Waals force). These are weak forces that don't require a lot of energy to overcome, so the boiling point is relatively low.

Boiling Point: Low.

E: \(CH_3CH_2CH_2CHO\) (Butanal)  

Butanal is an aldehyde. Aldehydes have a polar carbonyl group (C=O), which allows for dipole-dipole interactions between molecules. These interactions are stronger than the London dispersion forces in butane but still weaker than hydrogen bonding.

Boiling Point: Higher than butane but lower than alcohols and acids.

C: \(CH_3CH_2OCH_2CH_3\) (Ethyl Ether)

Ethyl ether has an ether group (-O-). Ethers have weak hydrogen bonding potential, where the oxygen can interact with hydrogen atoms of other molecules (e.g., water), but it doesn't form as strong hydrogen bonds as alcohols or acids. Ethyl ether also has London dispersion forces.

Boiling Point: Higher than butanal due to the ability to form some hydrogen bonds, though not as strong as alcohols and acids.

B: \(CH_3CH_2CH_2CH_2OH\) (Butanol)

Butanol has a hydroxyl group (-OH), which allows for strong hydrogen bonding between molecules. Hydrogen bonds are much stronger than dipole-dipole interactions and London dispersion forces, so butanol will have a significantly higher boiling point than butanal and ethyl ether.

Boiling Point: Higher than ether and aldehydes due to strong hydrogen bonding.

A: \(CH_3CH_2CH_2COOH\) (Butyric Acid)

Butyric acid has a carboxyl group (-COOH), which is capable of forming strong hydrogen bonds between molecules. These hydrogen bonds are particularly strong due to the polarity of the carbonyl group and the hydroxyl group in the carboxyl group, leading to a very high boiling point.

Boiling Point: The highest boiling point among the compounds listed, due to the strong hydrogen bonding.

Thus, the correct increasing order of boiling points is:  
D < E < C < B < A  which corresponds to Option 1.