Which of the following explains why the boiling points of hydrocarbons increase with increasing molar mass?
A. The larger mass makes molecules move slower, allowing for increased attractions.
B. Hydrogen bond strength increases
C. London forces become more pronounced with a greater number of atoms.

There are two correct answers to the question. The first correct answer is A, The larger mass makes molecules move slower, allowing for increased attractions. It is known that the larger the mass, the slower the molecules move. When this occurs, attractions between the molar mass increase.

The second correct answer is C, which states London forces become more pronounced with a greater number of atoms. London forces are attractive forces, which are temporary. They occur when the electrons of two atoms that are adjacent form dipoles which are also temporary. They are stronger with molecules that are very polarized.

The boiling points of hydrocarbon increase because of the following: the first is A and the second is C. Having a larger mass is known to make the molecules move slower. This will make sure that increased attractions are possible. There are different factors that will influence the boiling point.

The more carbons are available, the more that boiling points will increase. Branching is known to decrease the boiling point. There are various dispersion forces that may influence the various attractive forces depending on the functional groups that the hydrocarbon belongs to.