What happens to gas pressure if the temperature is increased while the volume is kept constant?

In a gas, the relationship between pressure, temperature, and volume 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 held constant. This means that as the temperature of the gas increases, the kinetic energy of the gas molecules also increases.

When the molecules have more energy, they move faster and collide with the walls of the container more frequently and with greater force. Since pressure is defined as the force per unit area exerted by gas molecules colliding with the walls of their container, an increase in both the frequency and force of these collisions leads to an increase in pressure.

Thus, when the temperature is raised while keeping the volume constant, the pressure will indeed increase, confirming why the correct choice is that the pressure increases.