Question

Regarding the kinetic molecular theory, which of the following statement is not true?

• A. The volume that gas molecules occupy is negligible compared to the volume within which the gas is contained
• B. There are no forces present between gas molecules
• C. Collisions between gas molecules are perfectly elastic
• D. Gas molecules travel in a continuous, random motion
• E. The average kinetic energy of gas molecules is inversely proportional to temperature

Answer 1

The correct option is E The average kinetic energy of gas molecules is inversely proportional to temperature

Kinetic model of gases, five assumptions are made:

1. Gases are made up of particles with no defined volume but with a defined mass. In other words their volume is miniscule compared to the distance between themselves and other molecules.
2. Gas particles undergo no intermolecular attractions or repulsions. This assumption implies that the particles possess no potential energy and thus their total energy is simply equal to their kinetic energies.
3. Gas particles are in continuous, random motion.
4. Collisions between gas particles are completely elastic. In other words, there is no net loss or gain of kinetic energy when particles collide.
5. The average kinetic energy is the same for all gases at a given temperature, regardless of the identity of the gas. Furthermore, this kinetic energy is proportional to the absolute temperature of the gas.