* Kinetic Energy and Temperature: The average kinetic energy of molecules is directly proportional to the absolute temperature. Higher temperatures mean higher kinetic energy.
* States of Matter:
* Gas: In the gas phase, molecules are far apart and have weak intermolecular forces (the forces of attraction between molecules). They move freely and randomly, colliding with each other and the container walls.
* Liquid: In the liquid phase, molecules are closer together than in a gas. They still move, but their motion is more restricted due to stronger intermolecular forces.
* Energy Required for Phase Changes: It takes energy to transition from a liquid to a gas (vaporization). This energy increases the kinetic energy of the molecules, allowing them to break free from the liquid's surface and enter the gas phase.
In summary: Because gas molecules have higher kinetic energy (due to weaker intermolecular forces and typically higher temperatures), they move faster than molecules in the liquid phase.
