* Constant Random Motion: Gas particles are in constant, random motion. They move in straight lines until they collide with each other or the walls of the container.
* Negligible Intermolecular Forces: The attractive forces between gas particles are very weak compared to the kinetic energy of the particles. This is why gases can expand to fill any container.
* Elastic Collisions: Collisions between gas particles and the container walls are perfectly elastic. This means that no kinetic energy is lost during the collision.
* Average Kinetic Energy Proportional to Temperature: The average kinetic energy of the gas particles is directly proportional to the absolute temperature of the gas. This means hotter gases have faster-moving particles.
* Occupy Entire Volume: The particles of a gas are spread far apart, and they move freely. This allows them to fill the entire volume of the container.
Important Note: These are general characteristics of ideal gases. Real gases exhibit deviations from ideal behavior, especially at high pressures and low temperatures, where intermolecular forces become more significant.
