What does Boyle's Law state about the relationship between pressure and volume of a gas at constant temperature?

Boyle's Law describes the relationship between the pressure and volume of a gas when the temperature remains constant. According to this law, as the volume of a gas decreases, the pressure increases, and conversely, when the volume increases, the pressure decreases. This means that pressure and volume are inversely proportional to each other under constant temperature conditions.

In practical terms, if you were to compress a gas in a sealed container, reducing its volume would cause the pressure to rise. Conversely, if you were to allow the gas to expand, the volume would increase and the pressure inside the container would drop. This inverse relationship is a foundational aspect of gas behavior, and it is crucial in many applications, such as in engines and various scientific experiments. Understanding this principle is essential for predicting how gases will behave under different conditions.