When the volume of a gas increases, what happens to its pressure?

When the volume of a gas increases, its pressure decreases due to the principles outlined in Boyle's Law, which states that the pressure of a gas is inversely related to its volume when temperature is held constant. This means that as the volume expands, the same number of gas molecules has more space to move around, leading to fewer collisions with the walls of the container per unit time. Since pressure is defined as force applied per unit area, a decrease in the frequency of collisions corresponds to a decrease in pressure.

When analyzing this concept, it’s essential to recognize that if the volume were to increase significantly, the density of the gas would decrease and the likelihood of molecules hitting the walls of their container would diminish, resulting in a drop in pressure. This relationship holds true in closed systems where the temperature is maintained constant, reflecting the direct application of gas laws in predicting behavior under changing conditions.