The kinetic molecular theory (KMT) of gases explains the behavior of gases based on the motion of their particles. Here are the main assumptions:
- Gas particles are tiny and far apart – The actual volume of gas particles is negligible compared to the volume of the container.
- Particles move randomly – Gas particles move in straight lines in all directions.
- No attractive or repulsive forces – Particles do not attract or repel each other.
- Elastic collisions – When gas particles collide with each other or the walls of the container, no energy is lost.
- Kinetic energy depends on temperature – The average kinetic energy of gas particles is directly proportional to the temperature in Kelvin.
In simple terms: Gas particles are tiny, move fast, bounce off each other perfectly, don’t stick together, and get faster as the temperature rises.