Question

according to the kinetic molecular theory, where does the pressure exerted by a gas in a container come from? select the correct answer below: pressure results from the average kinetic energy of the molecules being proportional to the temperature. pressure results from the molecules moving in straight lines. pressure results from the gas molecules being small. pressure results from collisions between the constantly moving gas molecules and the container walls.

Explanation:

According to the kinetic molecular theory, gas molecules are in constant motion. When these molecules collide with the walls of the container, they exert a force. Pressure is defined as force per unit area. So, the pressure exerted by a gas in a container comes from these collisions between the constantly - moving gas molecules and the container walls. The statement "Pressure results from the average kinetic energy of the molecules being proportional to the temperature" is related to the temperature - kinetic energy relationship in the theory but not directly to pressure. The fact that molecules move in straight lines (until they collide) is a general property of gas molecules in the theory but not the cause of pressure. And the size of gas molecules (gas molecules being small) is related to the assumption of negligible volume of gas molecules in the kinetic molecular theory, not to pressure.

Answer:

Pressure results from collisions between the constantly moving gas molecules and the container walls.