Kinetic Theory and Gas Pressure
The continuous bombardment of the gas molecules against the walls of the container results in an increase in gas pressure. According to the Kinetic theory of gases, the pressure at that point exerted by a gas molecule can be represented as,
P = 1/3ρ×c-2
where
- c is Mean Square Speed of a Gas Molecules
- ρ is Density of Gas
Suppose the container has n number of molecules of gas, with each of mass m, then the pressure can be represented as,
P = 1/3(nm/v)×c-2
where,
- V is Volume of Gas
Kinetic Theory of Gases
Kinetic Theory of Gases is a theoretical model which helps us understand the behavior of gases and their constituent particles. This theory suggests that gas is made up of a larger number of tiny particles which collide with each other and their surroundings and exchange kinetic energy between them. The kinetic theory of gases has various applications throughout physics, chemistry, and engineering and it is essential to understand many phenomena like diffusion, effusion, and Brownian motion.
In this article, we will learn about the assumptions of kinetic theory, its limitations, and others in detail.