Why does acetone have a lower boiling point than hexane? Why does acetone have a lower boiling point than hexane? I thought that since hexane is non-polar then it should have weaker intermolecular forces and a lower boiling point, but it doesn't. Why?

For reference, the boiling point of acetone is roughly 56 °C  while that of n-hexane is roughly 68 °C.
Hexane is a larger, longer-chain molecule so there are more London dispersion forces between n-hexane molecule which outweighs the dipole forces in acetone.