Question

Assumptions of Kinectic Molecular Theory of Gases .​

Answer 1

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The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the walls of the container, but otherwise do not interact; and (3) the transfer of kinetic energy between molecules is heat. These simplifying assumptions bring the characteristics of gases within the range of mathematical treatment.

The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the walls of the container, but otherwise do not interact; and (3) the transfer of kinetic energy between molecules is heat. These simplifying assumptions bring the characteristics of gases within the range of mathematical treatment.Such a model describes a perfect gas (q.v.) and is a reasonable approximation to a real gas, particularly in the limit of extreme dilution and high temperature. Such a simplified description, however, is not sufficiently precise to account for the behaviour of gases at high densities.

The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the walls of the container, but otherwise do not interact; and (3) the transfer of kinetic energy between molecules is heat. These simplifying assumptions bring the characteristics of gases within the range of mathematical treatment.Such a model describes a perfect gas (q.v.) and is a reasonable approximation to a real gas, particularly in the limit of extreme dilution and high temperature. Such a simplified description, however, is not sufficiently precise to account for the behaviour of gases at high densities.Based on the kinetic theory, pressure on the container walls can be quantitatively attributed to random collisions of molecules the average energy of which depends upon the gas temperature. The gas pressure can therefore be related directly to temperature and density. Many other gross properties of the gas can be derived, such as viscosity, thermal and electrical conduction, diffusion, heat capacity, and mobility. In order to explain observed deviations from perfect gas behaviour, such as condensation, the assumptions must be appropriately modified. In doing so, considerable insight has been gained as to the nature of molecular dynamics and interactions.

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Answer 2

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⤵answer⤵

Assumptions of Kinectic Molecular Theory of Gases .

▪Every gas is made up of a large no. of extremely small particles called molecules.

▪The molecules are considered as point masses as they are too small . Therefore, the total volume of the molecules is negligible as compared to the volume of the gas.

▪The molecules of the gas are in state of constant,rapid and random motion in all possible directions . The molecules move in a straight line until they collide with one another or with the walls of the container.

▪Under ordinary conditions of pressure and temperature , there exists no fires of attraction or repulsion between the molecules of gas and the molecules move independent of each other .

▪The pressure exerted by a gas is due to collision of molecules on the walls of the container .

▪The average kinectic energy of the molecules of the gas is directly proportional to the absolute temperature of gas .

▪There is no affect of gravity on the motion of molecules of the gas.

If it were so,the gas molecules will settle down at the bottom of the container which,intact,never happens .

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