As the temperature of a gas increases, what generally happens to its pressure if the volume is held constant?

When the temperature of a gas increases while the volume is held constant, the pressure of the gas increases. This relationship is described by Gay-Lussac’s law, which states that the pressure of a fixed amount of gas is directly proportional to its absolute temperature (measured in Kelvin) when the volume is unchanged.

As the temperature rises, the kinetic energy of the gas molecules increases. They move faster and collide more energetically with the walls of their container. Since the volume is constant, these more vigorous collisions result in increased pressure exerted by the gas on the walls of the container.

Understanding this principle is crucial in various applications, such as in understanding how pressure cookers work or in explaining the behavior of gases in various temperature conditions.