If the temperature of a gas increases, what happens to its pressure if the volume is kept constant?

When the temperature of a gas increases while keeping the volume constant, the pressure also increases. This relationship 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 (in Kelvin) when the volume is held constant.

As the temperature rises, the kinetic energy of the gas molecules also increases. This leads to more frequent and more forceful collisions of the gas molecules with the walls of the container, which results in an increase in the pressure exerted by the gas. Therefore, under the given condition of constant volume, an increase in temperature will indeed cause an increase in pressure.