What is typically true of the hydrocarbons with higher molecular weight?

Hydrocarbons with higher molecular weights typically have higher boiling points due to an increase in the number of carbon and hydrogen atoms in their molecular structure. As the molecular weight increases, the size of the molecules also increases, which leads to larger surface areas and stronger dispersion forces (also known as Van der Waals forces). These stronger intermolecular forces require more energy to overcome, resulting in higher boiling points.

It is important to note that while lower molecular weight hydrocarbons tend to be gases at room temperature or relatively volatile liquids, heavier hydrocarbons are more likely to exist as liquids or solids at room temperature. Hence, while options describing gaseous states or liquid states can be partially true, they do not give a complete picture of the relationship between molecular weight and physical properties such as boiling points.

Moreover, while reactivity can vary across different hydrocarbon classes, heavier hydrocarbons do not inherently have lower reactivity than lighter ones. Their chemical behavior is influenced by factors like branching, functional groups, and saturation rather than just molecular weight. Thus, option C captures the essence of how molecular weight correlates with boiling points in hydrocarbons.