Explain why ethers and alcohols of comparable molecular mass have different boiling points.

(N/A) Alcohols contain a polar $-OH$ group,which allows for the formation of intermolecular $H$-bonds between alcohol molecules. This association requires more energy to break during vaporization.
In contrast,ethers do not contain a hydrogen atom bonded directly to an oxygen atom,so they cannot form intermolecular $H$-bonds. Their intermolecular forces are primarily dipole-dipole interactions,which are weaker than $H$-bonds.
Therefore,for comparable molecular masses,alcohols have significantly higher boiling points than ethers.