Kinetic Theory of Gases Assumptions – Kinetic Theory of Gases

Kinetic Theory of Gases Assumptions – Kinetic Theory of Gases

We are giving a detailed and clear sheet on all Physics Notes that are very useful to understand the Basic Physics Concepts.

Assumptions of Kinetic Theory of Gases:
1. Every gas consists of extremely small particles known as molecules. The molecules of a given gas are all identical but are different from those of another gas.

2. The molecules of a gas are identical spherical, rigid and perfectly elastic point masses.

3. Their molecular size is negligible in comparison to intermolecular distance (10-9m).

4. The speed of gas molecules lies between zero and infinity (very high speed).

5. The distance covered by the molecules between two successive collisions is known as free path and mean of all free path is known as mean free path.

6. The number of collisions per unit volume in a gas remains constant.

7. No attractive or repulsive force acts between gas molecules.

8. Gravitational attraction among the molecules is ineffective due to extremely small masses and very high speed of molecules.

9. The density of gas is constant at all points of the vessel.

10. The molecules of a gas keep on moving randomly in all possible directions with all possible velocities.

Kinetic Theory of Gases:
In this concept, it is assumed that the molecules of gas are very minute with respect to their distances from each other. The molecules in gases are in constant, random motion and frequently collide with each other and with the walls of any container.

In this portion, you will learn about the properties of gases, based on density, pressure, temperature and energy. Continue reading here to learn more.

Kinetic Energy of an Ideal Gas Assumptions of Kinetic Theory of Gases
Gas Laws Ideal Gas Equation
Real Gases Degrees of Freedom
Mean Free Path Brownian Motion
Critical Temperature