The relationship between temperature and pressure is directly proportional, particularly in the context of gases. According to Gay-Lussac’s Law, if the volume of a gas is held constant, an increase in temperature will lead to an increase in pressure, and vice versa.
This means that when the temperature of a gas rises, the kinetic energy of its molecules increases, causing them to collide more frequently and with greater force against the walls of their container. As a result, the pressure increases. Conversely, if the temperature drops, the molecules move less vigorously, leading to fewer collisions and a decrease in pressure.
It’s important to note that this direct relationship holds true as long as the volume of the gas does not change. In situations where volume can vary, the relationship may not hold, and other gas laws such as Boyle’s Law and the Ideal Gas Law come into play.