"For a fixed amount of gas at a constant temperature, the pressure and volume are inversely proportional."
This means:
* As volume increases, pressure decreases.
* As volume decreases, pressure increases.
Example:
Imagine you have a sealed container of gas. If you increase the volume of the container (by making it bigger), the gas molecules will have more space to move around in. This means they will collide with the walls of the container less often, resulting in a lower pressure. Conversely, if you decrease the volume of the container, the gas molecules will have less space, collide more frequently, and exert a higher pressure.
Mathematical Expression:
Boyle's Law can be expressed mathematically as:
P₁V₁ = P₂V₂
Where:
* P₁ = Initial pressure
* V₁ = Initial volume
* P₂ = Final pressure
* V₂ = Final volume
Important Note:
Boyle's Law only applies to ideal gases at constant temperature. Real gases may deviate slightly from this law, especially at high pressures and low temperatures.
