What happens to the pressure of a gas if the temperature is increased while keeping volume constant?

When the temperature of a gas is increased while keeping the volume constant, the pressure of the gas increases. This behavior is described by Gay-Lussac's Law, which states that the pressure of a given mass of gas is directly proportional to its absolute temperature (measured in Kelvin) when the volume is held constant.

As the temperature rises, the kinetic energy of the gas molecules increases. This leads to more frequent and forceful collisions of the gas molecules with the walls of the container, resulting in higher pressure. Since the volume does not change, the only factor influencing the increase in pressure is the rise in temperature.

This relationship is fundamental in understanding how gases behave under different conditions and is crucial in various applications, such as in engines or pressure cookers, where controlling temperature and pressure is vital.