For a gas at constant volume, what happens to the pressure if the temperature is raised?

When a gas is kept at constant volume and its temperature is raised, the pressure of the gas increases. This relationship is described by Gay-Lussac's law, which states that the pressure of a gas is directly proportional to its absolute temperature (measured in Kelvin) when the volume is held constant.

At a constant volume, increasing the temperature causes the particles of the gas to gain kinetic energy. As these particles move faster, they collide with the walls of their container more frequently and with greater force. This increased frequency and intensity of collisions result in a higher pressure exerted by the gas on the walls of the container.

Therefore, as the temperature rises, the pressure responds by increasing, confirming the correct choice.