Question

What is kinetic gas theory?

Answer 1

The temperature of an ideal monatomic gas is proportional to the average kinetic energy of its atoms. The size of helium atoms relative to their spacing is shown to scale under 1950 atmospheres of pressure. The atoms have a certain, average speed, slowed down here two trillion fold from room temperature.

The kinetic theory describes a gas as a large number of submicroscopic particles (atoms or molecules), all of which are in constant rapid motion that has randomness arising from their many collisions with each other and with the walls of the container.

Kinetic theory explains macroscopicproperties of gases, such as pressure, temperature, viscosity, thermal conductivity, and volume, by considering their molecular composition and motion. The theory posits that gas pressure is due to the impacts, on the walls of a container, of molecules or atoms moving at different velocities.

Kinetic theory defines temperature in its own way, in contrast with the thermodynamic definition

Answer 2

Explanation

The molecule details regarding gases can be visualised with the help of Kinetic molecular theory of gases which is based on following assumptions.

(I) A gas consists of extremely small discrete identical particles, called the molecules, dispersed throughout the container.

(ii) Molecules are so small and so far apart that the actual volume of the molecules is negligible as compared to the total volume of gas.

(iii) Gas molecules are in constant random motion with high velocities. They move in straight lines with uniform speed and change directions on collision with other molecules or with the walls of container.

(iv) The intermolecular forces are negligible. Thus, the gas molecules can move freely, independent of each other.

(v) The effect of gravity on the motion of the molecules is negligible in comparison to the effect of collision.