Temperature is a vital factor that influences how gases behave. In the kinetic molecular theory, temperature is directly related to the average kinetic energy of the gas molecules. When the temperature of a gas increases, here's what happens:
- The molecules move faster owing to an increase in kinetic energy.
- This results in more frequent and more forceful collisions with the walls of the container.
When we refer to heating a gas at constant volume, we're saying the container's size doesn't change. So, as the gas's temperature rises, even if the space isn't expanding, the molecules still gain energy and collide more often. By experiencing more collisions, the pressure inside the container tends to increase if the volume is kept constant. This observation supports why statement (b) in the exercise is correct.