What happens to the pressure of a gas if the volume decreases while the temperature remains constant?

When the volume of a gas decreases while the temperature remains constant, the pressure of the gas must increase. This relationship is described by Boyle's Law, which states that for a given mass of an ideal gas at a constant temperature, the product of pressure and volume is a constant. Therefore, when the volume decreases, the same number of gas particles is forced into a smaller space, resulting in an increase in pressure.

In practical terms, if you were to compress a gas in a container while ensuring that the temperature doesn’t change (by allowing heat to escape or providing an equal amount of heat), you would observe that the gas molecules collide with the walls of the container more frequently and with greater force due to the reduced distance between them. This leads to a higher pressure.

This phenomenon is essential in understanding how gases behave under various conditions and is fundamental in multiple applications, including engines and gas storage systems.