Question

Which of the following statements about the kinetic molecular theory are not correct? O Attractive and repulsive forces between gas molecules are negligible The average kinetic energy of the molecules is not related to the absolute temperature Gases consist of molecules that are in continuous, random motion The combined volume of all the molecules of the gas is negligible relative to the total volume in which the gas is contained

Answer 1

Kinetic molecular theory clearly postulates the relation between Kinetic energy of Molecules to the absolute temperature. It states that:

The average kinetic energy is the same for all gases at a given temperature, regardless of the identity of the gas. Moreover this kinetic energy is proportional to the absolute temperature of the gas.

It relates kinetic energy of molecules to the absolute temperature by the equation:

here Kb is Boltzmann's constant (Kb = 1.38×10^-23 JK^-1)

T is the absolution temperature in kelvin

This equation says that with the rise in temperature, speed of molecules increases, and finally average kinetic energy of molecules increases.

So the incorrect statement about Kinetic Molecular Theory of gases is 2nd statement:

The average Kinetic Energy of the molecules is not related to absolute temperature.