What happens to the pressure of a gas in a rigid closed container as it is heated?

When a gas in a rigid closed container is heated, the temperature of the gas increases. According to the ideal gas law, there is a direct relationship between the temperature and pressure of a gas when the volume is held constant. Specifically, as the temperature rises, the kinetic energy of the gas molecules increases, leading to more collisions with the walls of the container. These more frequent and forceful collisions result in an increase in pressure.

This relationship is governed by Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature when the volume is constant. Therefore, heating the gas leads to a corresponding increase in pressure within the confined space of the container.