According to Boyle's Law, what is the relationship between pressure and volume?

Boyle's Law defines the relationship between pressure and volume in a gas when temperature is held constant. It states that the pressure of a gas is inversely proportional to its volume. This means that as the volume of a gas decreases, the pressure increases, provided the temperature does not change. This relationship can be mathematically expressed as P1V1 = P2V2, where P represents pressure and V represents volume.

In practical terms, if you were to compress a gas (decrease its volume), the molecules within the confined space will collide with the walls of the container more frequently, resulting in an increase in pressure. Conversely, if the volume increases, there is more space for the gas molecules to move around, leading to fewer collisions with the container walls and a decrease in pressure.

This understanding is critical in many applications involving gases, such as in pneumatic systems, where the manipulation of pressure and volume is essential for operation.

The incorrect options do not accurately capture the essence of Boyle's Law. It is not about pressure being equal in a confined volume or defining pressure as force intensity, nor is it that volume is directly proportional to pressure, which mischaracterizes their relationship.