Chemistry · States of Matter - Gases, Liquids and Solids

Hydrogen bonding is the deciding factor in the given options.Hydrogen bonding is not as extensive in ethanol as in water, and so its boiling point is lower than water's, despite its greater molecular weight.

Ethyl alcohol exhibits hydrogen bonding, but these bonds are not as strong as those in water. As a result, ethyl alcohol has a lower boiling point than water.

Diethyl ether is primarily influenced by London dispersion forces, which are weaker than the hydrogen bonds present in other options, resulting in a lower boiling point.

Water has strong hydrogen bonds, which require significant energy to break. This results in the highest boiling point among the given options.

Acetone experiences dipole-dipole interactions, which are stronger than London dispersion forces but weaker than hydrogen bonds in water, leading to a lower boiling point than water.