Diethyl ether C4H10O and butane C4H10 have different intermolecular forces that affect their boiling points. Diethyl ether has a polar oxygen atom, which leads to the presence of dipole-dipole interactions in addition to the London dispersion forces induced dipole-induced dipole interactions that are present in both molecules. Butane, on the other hand, is a nonpolar molecule and only experiences London dispersion forces.Since dipole-dipole interactions are stronger than London dispersion forces, diethyl ether is expected to have a higher boiling point than butane due to the additional intermolecular forces present in its structure. In practice, this prediction holds true: the boiling point of diethyl ether is approximately 34.6C 94.3F , while the boiling point of butane is approximately -0.5C 31.1F .