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Which of the following statements concerning gas pressure is/are correct? (1) Gas pressure arises from gas molecules sticking to the wall of the container holding the gas. (2) The force exerted on the inside walls of a gas-filled container is inversely proportional to the number of gas molecules within the container. (3) As the temperature of a gas increases, gas molecules exert more force on the walls of their container.

Answer :

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Answer:

As the temperature of a gas increases, gas molecules exert more force on the walls of their container.

Explanation:

Pressure is the force exerted by a substance per unit area on another substance. The pressure of a gas is the force that the gas exerts on the walls of its container.

Gases collide frequently with each other and the walls of the container. This pressure of the gas increases with increase in temperature since increase in temperature increases the kinetic energy of gas molecules. They now collide more frequently with the walls of the container hence the answer.

The gas pressure is defined as the force exerted by the gas particles when they collide with the walls of the container. It is the pressure exerted per unit area.

The correct option is:

Option C. As the temperature of a gas increases, gas molecules exert more force on the walls of their container.

The correct explanation can be given as:

  • The gas molecules are in random motions, and continuously exert pressure on the walls of the container.

  • As the temperature rises, the kinetic energy of the particles is also increased, which causes a faster collision.

  • Thus, the gas pressure is increased as the temperature is increased.

Therefore, option C is correct.

To know more about gas pressure, refer to the following link:

https://brainly.com/question/18124975

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