Which statement below is not a premise of the Kinetic-molecular theory of gases?

a. Gas particles are extremely small and have relatively large distances between them.

b. Gas particles are continuously moving in random, straight-line motion as they collide with each other and the container walls.

c. The average kinetic energy of gas particles is proportional to the temperature of the gas.

d. All are premise of KMT.

Question

Chemistry

Demarcus Thompson

3 July, 02:20

Which statement below is not a premise of the Kinetic-molecular theory of gases?

a. Gas particles are extremely small and have relatively large distances between them.

b. Gas particles are continuously moving in random, straight-line motion as they collide with each other and the container walls.

c. The average kinetic energy of gas particles is proportional to the temperature of the gas.

d. All are premise of KMT.

+5

Answers (1)

Know the Answer?

Vanessa Farrell · Answer 1

d = all are premise of KMT.

Explanation:

A

Gas particles are extremely small and have relatively large distance between them.

B

Gas particles are continuously moving in random, straight-line motion as they are collide with each other and the container walls.

C

The average kinetic energy of gas particles is proportional to the temperature of gas.

All these are the premise of kinetic molecular theory. According to kinetic molecular theory, the particles pf gases are very small and randomly move in the available space. They move freely in straight line and colloid with each other and also the wall of container. This collision is elastic. As molecules strike with each other and walls of container their energy increases, and they gets warmer. So their kinetic energy is proportional to the temperature because mass of particle is constant.