Which rule is described by the kinetic molecular theory? gas particles attract one another and bond together gas particles collide and there is an energy transfer between molecules gas particles cannot be compressed the speed of gas particles is directly proportional to the temperature

The kinetic molecular theory describes gases as consisting of tiny particles in constant, straight-line motion that frequently collide with one another and with the walls of their container in elastic collisions (meaning there is an energy transfer between molecules). Therefore, the rule that best aligns with the kinetic molecular theory is: "gas particles collide and there is an energy transfer between molecules" Here’s why the other choices are not consistent with the kinetic molecular theory: • "gas particles attract one another and bond together" – The kinetic molecular theory treats gas particles as having negligible intermolecular forces (except during collisions), and gases generally do not form bonds. • "gas particles cannot be compressed" – Gases are compressible because there is a significant amount of empty space between particles; the particles themselves are very small relative to the distances between them. • "the speed of gas particles is directly proportional to the temperature" – While the average kinetic energy of gas particles is directly proportional to the temperature, the relationship between the speed and temperature is given by v ∝ √T rather than being directly proportional. Thus, the correct statement is the one about collisions and energy transfer.