Question

postulates of kimetic theory of gases

Answer 1

Heya,

Answer to your question is:-

Postulates of the Kinetic Theory of Gases.

1.The molecules in a gas are small and very far apart. Most of the volume which a gas occupies is empty space.

2.Gas molecules are in constant random motion. Just as many molecules are moving in one direction as in any other.

3.Molecules can collide with each other and with the walls of the container. Collisions with the walls account for the pressure of the gas.

4.When collisions occur, the molecules lose no kinetic energy; that is, the collisions are said to be perfectly elastic. The total kinetic energy of all the molecules remains constant unless there is some outside interference with the

5.The molecules exert no attractive or repulsive forces on one another except during the process of collision. Between collisions, they move in straight lines.

HOPE THIS HELPS YOU:-))
@Ashu

Answer 2

Hello!!

The microscopic theory of gas behavior based on molecular motion is called the kinetic theory of gases.

 Postulates of the Kinetic Theory of Gases.

1      The molecules in a gas are small and very far apart. Most of the volume which a gas occupies is empty space.

2      Gas molecules are in constant random motion. Just as many molecules are moving in one direction as in any other.

3      Molecules can collide with each other and with the walls of the container. Collisions with the walls account for the pressure of the gas.

4      When collisions occur, the molecules lose no kinetic energy; that is, the collisions are said to be perfectly elastic. The total kinetic energy of all the molecules remains constant unless there is some outside interference with the

5      The molecules exert no attractive or repulsive forces on one another except during the process of collision. Between collisions, they move in straight lines.

 

From them it is possible to derive the following expression for the pressure of a gas in terms of the properties of its molecules:


P=1N3Vm(u2)ave
(9.12.1)(9.12.1)
P=1N3Vm(u2)ave

      


Where P, V = pressure and volume of the gas

              N = number of molecules

              m = mass of each molecule

       (u2)ave = average (or mean) of the squares of all individual molecular velocities. This mean square velocity must be used because pressure is proportional to the square of molecular velocity, and molecular collisions cause different molecules to have quite different velocities.

Rather than concerning ourselves with the procedure for deriving let us inspect the equation and see that its general features are much as we would expect. In some ways, the ability to do this with a formula is more useful than the ability to derive it.    



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