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Based on the kinetic molecular theory, which of the following statements is correct about a sample of gas at a constant temperature and volume?
A) The net kinetic energy of its particles decreases due to collisions.
B) The net kinetic energy of its particles increases due to collisions.
C) It has a constant average kinetic energy.
D) Its average kinetic energy is always zero

Respuesta :

skyluke89

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:

[tex]KE=\frac{3}{2}kT[/tex]

where

KE is the kinetic energy

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.

Learn more about ideal gases:

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#LearnwithBrainly

BlueGhirahim

Answer:

B. There is negligible force of attraction between them.

Explanation:

I took the test :)

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