If the pressure of a gas increases while its volume remains constant, what happens to its temperature?

When the pressure of a gas increases while its volume remains constant, its temperature must also increase. This relationship is described by Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature when the volume is kept constant.

According to this principle, if you increase the pressure of a gas by applying more force externally (for example, by compressing the gas in a sealed container), the kinetic energy of the gas molecules increases, which directly correlates to an increase in temperature. This is because the molecules collide with the walls of the container more frequently and with greater energy as they are under higher pressure.

Thus, the correct understanding is that an increase in pressure at constant volume pulls the temperature up, leading to the conclusion that the temperature increases in this scenario.