n-Butane, Propan-1-ol, Propanal, Acetone, Methoxymethane ( increasing order of boilingpoint)

To determine the increasing order of boiling points for the given compounds, we need to consider their molecular structures and intermolecular forces.

1. Methoxymethane (CH3OCH3): This compound is a type of ether. It has a relatively low boiling point due to its weak intermolecular forces, specifically London dispersion forces.

2. Propanal (CH3CH2CHO): Propanal is an aldehyde. It has a slightly higher boiling point compared to methoxymethane because it can form stronger dipole-dipole interactions due to the presence of the carbonyl group.

3. Acetone (CH3COCH3): Acetone is a ketone. It has a higher boiling point than propanal because it has a larger molecular size and can form stronger dipole-dipole interactions.

4. Propan-1-ol (CH3CH2CH2OH): Propan-1-ol is an alcohol. It has the highest boiling point among the given compounds due to the presence of hydrogen bonding. Hydrogen bonding is a strong intermolecular force that occurs between the hydrogen atom of one molecule and the oxygen atom of another molecule.

5. n-Butane (CH3CH2CH2CH3): n-Butane is an alkane. It has the highest molecular weight among the given compounds but lacks any functional groups that can form strong intermolecular forces. Therefore, it has the highest boiling point.

So, the increasing order of boiling points for the given compounds is: Methoxymethane < Propanal < Acetone < Propan-1-ol < n-Butane.