What happens to the pressure of a gas as its volume decreases at constant temperature?

When a gas is confined to a smaller volume at constant temperature, the pressure of the gas increases due to the principles outlined in Boyle's Law. This law states that for a given mass of gas at a constant temperature, the pressure of the gas is inversely proportional to its volume. Mathematically, this relationship can be expressed as PV = k, where P represents pressure, V is the volume, and k is a constant.

As the volume decreases, the same number of gas molecules is forced into a smaller space, leading to more frequent collisions between the gas molecules and the walls of the container. This increased frequency of collisions results in a higher pressure. Therefore, when the volume of a gas decreases while maintaining a constant temperature, you can expect the pressure to increase significantly.

In this case, the answer is supported by the direct relationship described by Boyle’s Law, confirming that a reduction in volume leads to an increase in pressure when temperature is held constant.