Arrange the following in order of increasing boiling points :
(i) propanone (ii) propanal (iii ) propan -1 ol (iv ) Propane ( v ) Dimethyl ehter

Explanation

To arrange the compounds in order of increasing boiling points, we need to consider the types of intermolecular forces present in each compound. The boiling point is influenced by the strength of these forces, with hydrogen bonding being the strongest, followed by dipole-dipole interactions, and finally London dispersion forces.

Let's analyze each compound:

1. **Propane (C3H8)**: This is a non-polar molecule and exhibits only London dispersion forces. It will have the lowest boiling point among the given compounds.

2. **Dimethyl ether (C2H6O)**: This compound has a polar C-O bond, leading to dipole-dipole interactions. However, it does not have hydrogen bonding, so its boiling point will be higher than that of propane but lower than those of alcohols and aldehydes.

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