Alcohols have higher boiling points than ethers of the same molecular mass due to hydrogen bonding.

Solution

Chemistry ma’am · 3 steps

Look for the O–H: ethanol has one, dimethyl ether does not, and that one bond is the whole story.

1. Same mass, fair test. Compare ethanol, C₂H₅OH, with dimethyl ether, CH₃OCH₃. Both have molar mass 46 g mol⁻¹, so their London forces are about the same size.

   Compound	O–H bond?	Strongest force between molecules	Boiling point
   C₂H₅OH (alcohol)	yes	intermolecular hydrogen bonding	78 °C
   CH₃OCH₃ (ether)	no	dipole–dipole only	-24 °C

2. Why ethers miss out. A hydrogen bond needs an H atom attached to O, N or F. In an ether every H sits on carbon, so ether molecules cannot hydrogen bond to each other. They have only weak dipole–dipole attraction.
3. So. Alcohol molecules are held together by hydrogen bonds, and boiling needs extra energy to break them. The statement is true.

The idea to keep. When molar masses match, check which molecule has H on O, N or F. That molecule hydrogen bonds to its own kind and boils higher.

Answer from the NTA final answer key. Solution by PrepWiser.