1-Butanol has a higher boiling point than diethyl ether because of stronger intermolecular forces. 1-Butanol is a primary alcohol, which means that it has a hydroxyl group (-OH) bonded to a primary carbon atom. Diethyl ether is an ether, which means that it has an oxygen atom bonded to two alkyl groups. The hydroxyl group in 1-butanol can form hydrogen bonds with other hydroxyl groups and with the hydrogen atoms on the carbon atoms. These hydrogen bonds are stronger than the van der Waals forces that are present in diethyl ether. The stronger hydrogen bonds in 1-butanol lead to a higher boiling point.

Here is a table summarizing the boiling points of 1-butanol and diethyl ether:

| Compound | Boiling Point (°C) |

|---|---|

| 1-Butanol | 117.7 |

| Diethyl ether | 34.5 |

As you can see, 1-butanol has a much higher boiling point than diethyl ether. This difference in boiling points is due to the difference in intermolecular forces between the two compounds.