When a gas in a container of fixed volume is heated, the molecules of the gas experience an increase in kinetic energy. This increase in kinetic energy leads to several effects on the gas molecules:
Increased Speed: As the gas molecules gain kinetic energy, they move faster. The average speed of the molecules increases, resulting in a higher root mean square (rms) velocity. This increased speed leads to more frequent and energetic collisions between molecules.
Increased Collisions: With higher kinetic energy, the gas molecules collide with each other and the walls of the container more frequently. These collisions result in an increased pressure inside the container.
Increased Vibration and Rotation: The additional energy provided by heating can also cause the gas molecules to vibrate and rotate more vigorously. These vibrational and rotational motions contribute to the overall internal energy of the gas.
Expansion: Heating a gas in a fixed-volume container will increase the pressure inside the container due to increased collisions. If the container is rigid and unable to expand, the pressure will continue to rise. However, if the container is flexible or open, the increased pressure may cause the gas to expand and occupy a larger volume.
It's important to note that the behavior of the gas molecules is described by the ideal gas law, which assumes an idealized scenario where the gas particles have negligible volume and interact only through elastic collisions. In reality, intermolecular forces and the specific properties of the gas can affect its behavior to some extent.