The boiling point of n-butane, a measure of its tendency to vaporize, is influenced by intermolecular forces. These forces, which include van der Waals interactions and dipole-dipole interactions, resist the separation of molecules and contribute to the liquid state. As temperature increases, the kinetic energy of molecules overcomes these forces, leading to vaporization. The boiling point of n-butane at standard atmospheric pressure is -0.5°C (31.5°F).
