Kinetic Theory

Kinetic Molecular Theory

Kinetic molecular theory was proposed by Rudolf Clausius to describe the nature of gas molecules. According to the theory, gases are composed of large number of molecules. Here Nobel gases are supposed to be composed of atoms, rather than molecules. These molecules or atoms are moving continuously in random manner. Please express your views of this topic Equation for Kinetic Energy by commenting on blog.

Since two molecules or atoms in gases are spaced apart from each other, they move in a straight line until they collide with other molecules or atoms or with wall. The theory also considers the collisions to be binary which means that only two molecules or atoms are involved in the collision. According to the theory, molecular volume of gas is negligible as compared to total gas volume in a container.
However, this assumption fails when the number of molecules in a gas increases up-to 1 mol/lit. Due to increased number of molecules, the molecular volume of gas cannot longer be considered as negligible as compared to the container volume. The theory also assumes that attractive forces between molecules or atoms are negligible.

Kinetic Theory
The kinetic theory is also known as kinetic molecular theory that explains almost all the basic law’s of matter namely Charles’ law, Boyle’s law etc.

Kinetic Theory of Matter

The kinetic theory of matter explains the heat transfer of heat flow and also explains relation between pressure, temperature and volume of gases.

Kinetic Molecular Theory of Gases

According to kinetic molecular theory, gases have large number of molecules that are moving continuously in a straight line till they collide with other molecules or with container’s wall. The theory assumes the molecular volume and attractive forces between gas molecules negligible. Hence under constant gas temperature, the average kinetic energy of gas molecules also remains constant.
This is due to the fact that the collisions are elastic that can cause energy transfer but not energy loss. The average kinetic energy of gas molecules depends on temperature of gas. Hence at a particular temperature, average kinetic energy of molecules of all gases will be same irrespective of their shape, size or weight.

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Kinetic Theory of Gases

The kinetic theory of gases explains the nature of gases. According to the theory, all gases are made up of molecules that are in continuous and random motion. Owing to large distance between two molecules of a gas, these molecules move in straight line till any collision. All the collisions are elastic and hence do not cause any energy loss.
There is no attraction or repulsion force acting between gas molecules. At lower molecular concentration, the molecular volume of gas can be considered negligible as compared to the total container’s gas volume.