hich of the following assumptions of the kinetic molecular theory of gases is not valid for real gases at high pressure? a. the volume of the gas particle is much smaller than the distance between the gas particles. b. the gas particles behave like hard, spherical objects in a state of constant motion. c. the average kinetic energy of the gas particle depends upon the temperature of the gas only. d. the gas particles move in a straight line until they collide with another particle or the walls of the container. e. all of the above are valid for real gases at high pressures

Solution: The energy of a molecule does not change when it collides with a container's walls, according to the kinetic theory of gases. Therefore, the assumption is false With the aid of step-by-step solutions offered by experts, you can dispel your concerns and obtain favorable exam results.

The kinetic-molecular theory of gases postulates that ideal gas molecules are perpetually in motion, have a minimal volume, negligible intermolecular interactions, endure collisions that are perfectly elastic.

Keep in mind that ideal gas models are ineffective at low temperatures and high pressures because the gas expands at these conditions.

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