What is the relationship between pressure, volume, and temperature in a gas described by Boyle's Law?

Boyle's Law describes the relationship between the pressure and volume of a gas at constant temperature. According to this law, when the pressure of a gas increases, the volume decreases, and conversely, when the pressure decreases, the volume increases, provided the temperature remains unchanged. This is an inverse relationship, which can be mathematically represented by the equation ( P \times V = k ), where ( k ) is a constant.

This means that if you take a fixed amount of gas and compress it (increasing the pressure), the volume will shrink. Conversely, if you allow the gas to expand (decreasing the pressure), the volume will increase. The emphasis on temperature being constant is crucial; any changes in temperature would affect this relationship as described by other gas laws, such as Charles's Law. This fundamental understanding of gas behavior is important in HVAC applications, where managing pressure and volume is key to system efficiency and effectiveness.