Question

At the molecular level explain the energy changes when liquid acetone is converted to a vapor at its boiling point.

Answer 1

When in liquid state, acetone has hydrogen bonding, london dispersion forces, and polarity interactions (dipole-dipole).

When adding energy in the form of internal energy, you are "breaking" or "loosening" those forces

London dispersion forces will be almost 0. The Hydrogen bonding is not enough to mantain molecules in liquid state. The dipole-dipole is loose enough to let molecules vibrate, translate, and move at high speeds.

The energy is increasing the average kinetic energy of the molecules, they move faster, they crash way more than in liquid state

In gas, there is an extreme change in volume (1:1000)