Based on the kinetic molecular theory, which of the following statements is correct about a sample of gas at a constant temperature and volume?

The net kinetic energy of its particles decreases due to collisions.

The net kinetic energy of its particles increases due to collisions.

It has a constant average kinetic energy.

Its average kinetic energy is always zero.

Question

Chemistry

Snow

6 October, 12:40

Based on the kinetic molecular theory, which of the following statements is correct about a sample of gas at a constant temperature and volume?

The net kinetic energy of its particles decreases due to collisions.

The net kinetic energy of its particles increases due to collisions.

It has a constant average kinetic energy.

Its average kinetic energy is always zero.

+1

Answers (1)

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Naima Nicholson · Answer 1

C) It has a constant average kinetic energy

Explanation:

The average kinetic energy of the particles in a gas is directly proportional to the temperature of the gas, according to the equation.

k is the Boltzmann's constant

T is the absolute temperature of the gas

Therefore, temperature of a gas is a measure of the average kinetic energy of the particles.

In this problem, we are told that the gas is at constant temperature (and volume) : therefore, according to the previous equation, this means that the average kinetic energy is also constant.