The molar enthalpy of vaporisation of acetone is less than that of water. Why?

(N/A) The amount of heat required to vaporise one mole of a liquid at constant temperature and under standard pressure $(1 \ bar)$ is called its molar enthalpy of vaporisation,denoted as $\Delta_{vap} H^{\ominus}$.
The molar enthalpy of vaporisation of water is higher than that of acetone because there is strong intermolecular hydrogen bonding present in $H_{2}O$ molecules,whereas acetone molecules are held together by weaker dipole-dipole interactions.