Question

According to the kinetic theory of gases:
(This question has multiple correct options)
A) Pressure of a gas is due to collisions of molecules with each other.
B) Kinetic energy is proportional to the square roots of the temperature.
C) Pressure of a gas is due to collisions of molecules against the sides of the container.
D) There is no force of attraction between molecules.

Answer 1

Hint:Thermodynamic behavior of gases includes a large number of identical submicroscopic particles, atoms, or molecules all of which are in constant, and random motion. They also undergo random elastic collisions between themselves and also with the enclosing walls of the container. Also, there are no interactive forces between the particles.

Complete step by step answer:

The kinetic theory of gases is a model of the thermodynamic behavior of gases. This model describes a gas as a large number of identical submicroscopic particles, atoms, or molecules all of which are in constant, and random motion and whose size is considered as much smaller than the average distance between the particles. These molecules undergo random elastic collisions between themselves and also with the enclosing walls of the container. As the collisions are perfectly elastic the molecules are considered to be perfectly spherical in shape and elastic in nature and the total kinetic energy of all the molecules remains constant.
These random collisions with the walls and between themselves account for the pressure of the gas. If the molecules move faster, they will exert a greater force on the container each time they hit the walls or each other, which further leads to an increase in the pressure. Except during the process of collision, the molecules exert no attractive or repulsive forces on each other, which means there are no interactive forces between the particles. During collisions between themselves, or with the wall, they move in straight lines.
The correct answer is option A, C, and D.

Note:
But, always remember that the average kinetic energy for the particles in a gas sample is proportional to the temperature, or proportional to the absolute temperature, which means if we double the temperature the kinetic energy will be doubled.