In this article we will write an article we will have a brief discussion the Kinetic theory of gases. This article will give all the information which is required to understand the Kinetic theory of gases. The kinetic theory of gases is a theory which explains the behaviour of a hypothetical gas known as the Ideal Gas or Perfect Gas.
What Does this Theory Say?
The Kinetic theory of gases tells that the particles are in continuous random motion and collide with each other and also with the walls of the container. The collisions that takes place are elastic which means there is no loss in the energy because of which both total kinetic energy and total momentum are reserved. This theory works under some assumptions. The assumptions are as follows.
Assumptions of Theory:
- Gases consist of small particles of matter that are in constant motion.
- The particles constantly collide with each other and with the walls of the container. The collision that takes place are elastic in nature that means there is no loss in energy.
- The gas particles are separated with a large distance which is greater than the size of the particle.
- There is no attraction or repulsion between the particles.
- The speed of the gas particles are dependent on the temperature of the gas.
Some of the physical properties of gases are explained by this model. We know that the most of the space in a gas is empty therefore it possesses low density and can expand or contract under external influence. From the above point that the particles are in constant motion means that they always mix with each other.
Understanding the Ideal Gas
Let us understand what an ideal gas is. An Ideal gas is that which follows the statement of Kinetic theory. Practically real gases are not ideal but there are some gases which are nearly ideal. As ideal gases do not really exist but the Kinetic theory help us to model an ideal gas.
The Ideal Gas equation
An ideal gas can be expressed as an equation mathematically. The equation of the ideal gas is given as follows
Where P is pressure in atmosphere, V is volume in Litters, ‘n’ is number of moles of gas present, R is a constant and its value is 0.0821 atm.L/mol.K, T is temperature in Kelvin. This ideal gas law relates the pressure, temperature, volume and number of moles of ideal gas. Here R is known as universal gas constant.