According to Gay-Lussac's Law, what happens to the pressure of a gas if the temperature increases while the volume remains constant?

Gay-Lussac's Law states that the pressure of a given mass of gas is directly proportional to its absolute temperature when the volume is held constant. This means that as the temperature of the gas increases, the kinetic energy of the gas molecules also increases, leading to more frequent and more forceful collisions with the walls of the container. As a result, the pressure of the gas rises.

When the volume remains constant, any increase in temperature translates directly to an increase in pressure. This principle can be observed in practical scenarios, such as a sealed, pressurized container being heated. As the temperature of the gas inside the container rises, the pressure inside the container also rises due to the increased energy and movement of the gas particles.

Thus, when the temperature increases with volume held constant, the pressure necessarily increases, making this the correct interpretation of Gay-Lussac's Law.