The Kinetic Molecular Theory (KMT) of gases is a model that explains the behavior of gases based on the idea that gases are made up of tiny particles (atoms or molecules) that are in constant motion. Here are the main points:
- Gas particles are in constant, random motion.
- They move in straight lines until they collide with each other or the walls of their container.
- Gas particles are very far apart compared to their size.
- Most of the volume of a gas is empty space, which is why gases can be compressed easily.
- Collisions are perfectly elastic.
- When gas particles collide with each other or with the walls of a container, no energy is lost; it just transfers from one particle to another.
- There are no attractive or repulsive forces between gas particles.
- Gas particles move independently of one another, except during collisions.
- The average kinetic energy of gas particles depends on temperature.
- The higher the temperature, the faster the particles move, and the more energy they have.
In short: Gases are made of tiny, constantly moving particles, collisions don’t lose energy, and temperature controls how fast they move.