Question

Which of the following is NOT true in the kinetic molecular theory of ideal gases?

The size of the molecules are negligible compared to the volume of the container

The kinetic energy of a sample is proportional to the temperature of the gas.

Collisions are elastic (no friction occurs between the molecules when they collide)

The pressure of a sample is affected by which gases are present.

AND WHY?

Answer 1

Below are the Assumptions of Kinetic theory of gases;

A) Gases particles (molecules or atoms) are in constant random motion.

B) Gas particles are constantly colliding with each other and the walls of their container. These collisions are elastic and hence no loss of energy.

C) Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.

D) There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.

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

As per assumption (D), below is false;

The pressure of a sample is affected by which gases are present.