Kinetic theory of gases – assumptions

The simplest kinetic model is based on the assumption that: (1) a gas is composed of a large number of identical molecules moving in a straight line, separated by large distances relative to their size; (2) molecules collide in absolute (do not lose) energy alone with the walls of the vessel, but not in contact; and (3) kinetic energy transfer between heat molecules. This assumption makes it easier to bring the gas features within the mathematical treatment range.

Such a model defines perfect gas and is a reasonable measurement of real gas, especially at the extremes of purification and high temperatures. Such a simplified explanation, however, is not accurate enough to follow the behavior of gases where it is too crowded.

THEORY

Kinetic theory of gas is a theater model that describes the formation of gas cells in terms of a large number of small particles that include atoms and molecules. In addition, the theory states that gas pressure arises as a result of colliding particles and vessel walls. Kinetic theory of gas also defines features such as temperature, volume, pressure and transport properties such as viscosity and thermal conductivity as well as high distribution. It basically describes all the aspects associated with a minor event.

Theoretical significance is that it helps to improve the correlation between macroscopic structures and the microscopic phenomenon. In simple terms, gas kinetic theory also helps us to learn the action of molecules. In general, gas molecules are constantly moving and often collide with the walls of containers. In addition, the model also helps in understanding related events such as the Brownian movement.

Based on the kinetic concept, the pressure on the walls of the containers may be specified by the degree of random collision of the existing medium energy molecules depending on the temperature of the gas. Gas pressure can therefore be directly related to temperature and congestion. Many other serious gaseous substances can be found, such as viscosity, thermal conductivity, distribution, thermal energy, and mobility. In order to explain the observed deviations in total gas behavior, such as summarizing, the guess must be adjusted accordingly. In doing so, a great deal of understanding has been gained regarding the nature of cellular mutations and interactions.

Kinetic Theory of Gases Postulates

The kinetic theory of gas postulates helps to understand macroscopic structures from small structures.

Gases contain a large number of tiny particles (atoms and molecules). These particles are very small compared to the distance between the particles. The size of each particle is considered to be insignificant and most of the gas-containing volume is empty.

These molecules are constantly moving randomly, causing them to collide with the walls of the vessel. As gas molecules collide with vessel walls, molecules transmit pressure to the walls. Basically, this results in the production of immeasurable energy. Therefore, when we divide this force by space it is defined as pressure.

The collision between the molecules and the walls extends completely. That means that when molecules collide they do not lose kinetic energy. Molecules never slow down and will stay at the same speed.

The kinetic energy in the middle of the gas particles also changes with temperature. that is, When the temperature is high, it increases the kinetic energy level of the gas.

Molecules do not have the ability to attract or compete unless they collide.

ACCORDING TO KINETIC THEORY OF GASES

a) In line with the postulate kinetic theory of gases, the friction between molecules and the wall of the container expands completely naturally.

(b) When a mass  of gas m traveling at high speed collides with the wall of a container, the pressure change is Δp = – 2mu. Therefore, a heavy molecule will transfer more pressure to the wall as there will be a significant change in the pressure of the colliding gas molecule. However, this is not set in kinetic theory.

(c) According to Maxwell-Boltzmann of molecular speed, very few molecules have a high or very low speed. Most molecules move at a moderate speed.

(d) According to the kinetic theory of gases, a gas molecule moves in a straight line unless it collides with another molecule or in a container wall and a change in pressure is seen only after a collision.

CONCLUSION

The kinetic theory of gas describes the three macroscopic aspects of gas in terms of the small size of the atoms and molecules that make up gas. In general, the physical properties of solids and liquids can be defined by their size, shape, size, volume etc. However, in the case of gases, they do not have a precise shape, size, size, or volume. Kinetic theory of gas is useful and can be used in this regard.

With the help of kinetic gas theory, the physical properties of any gas can be generally described in terms of three measurable macroscopic objects. Pressure, volume and temperature of the container in which the gas is stored or located.