The boiling point of a compound is determined by the strength of its intermolecular forces. Compounds with different polarities can have different boiling points, even if they have the same molar mass. Compound B, which has polar C-O bonds, would have a higher boiling point than compound A, which has nonpolar C-H bonds.
The boiling points of compounds depend on the strength of the intermolecular forces between their molecules. In this case, we have two compounds with the same molecular formula (C7H16) and molar mass, but different boiling points. The compound with the higher boiling point will have stronger intermolecular forces, which can be attributed to differences in polarity.
Compound A:
Compound A has a structure similar to 2-methylpropane, which contains nonpolar C-H bonds. These bonds have similar electronegativities and result in a small dipole moment. Therefore, Compound A will have a low boiling point compared to the other compound.
Compound B:
Compound B has a structure similar to ethyl methyl ether, which contains polar C-O single bonds. These bonds have a significant dipole moment due to the difference in electronegativity between carbon and oxygen. As a result, Compound B will have a higher boiling point compared to Compound A.
The difference in boiling points is due to the different strength of intermolecular dipole-dipole interactions caused by the polarity of the compounds.