The kinetic theory of gas is a model that describes the behavior of gases at a molecular level. According to this theory, gases are made up of large numbers of tiny particles (atoms or molecules) that are in constant, random motion. The particles move in straight lines until they collide with each other or with the walls of the container.
Key assumptions of the kinetic theory of gas include:
1. Gas particles are tiny and have negligible volume compared to the volume of the container they are in.
2. Gas particles are in constant, random motion.
3. Gas particles collide with each other and with the walls of the container, resulting in pressure.
4. Gas particles obey Newton's laws of motion.
5. The average kinetic energy of gas particles is proportional to the temperature of the gas.
This theory helps explain various properties of gases, such as pressure, temperature, volume, and diffusion, by considering the behavior of individual gas particles.
What is a kinetic theory of gas
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