$$ \begin{array}{|l|c|c|} \hline \text{Name} & \text{Molecular} & \text{Molar Mass} \\ & \text{Formula} & \text{(g/mol)} \\ \hline \text{Ethane} & \ce{C2H6} & 30 \\ \hline \text{Butane} & \ce{C4H10} & 58 \\ \hline \end{array} $$

The molecular formula and molar mass of two straight-chain hydrocarbons are listed in the table above. Based on the information in the table, which compound has the higher boiling point, and why is that compound's boiling point higher?

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Both ethane and butane are nonpolar molecules due to their symmetrical geometry. Both do not form hydrogen bonds or dipole-dipole attractions.

All molecules have dispersion forces, which are caused by random movement of electrons. Dispersion forces are stronger in larger molecules due to larger electron clouds.