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Question

According to the kinetic theory of gases:

A
Pressure of a gas is due to collisions of molecules with each other
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B
Kinetic energy is proportional to square root of the temperature
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C
Pressure of a gas is due to collisions of molecules against the sides of the container
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D
There is no force of attraction between gas molecules
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Solution

The correct options are
A Pressure of a gas is due to collisions of molecules against the sides of the container
B There is no force of attraction between gas molecules
C Pressure of a gas is due to collisions of molecules with each other

Postulates of 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.

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.

Hence options A,C & D are correct.


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