Boyle's law
Boyle's Law (pronounced: /bɔɪlz lɔː/) is a fundamental principle in physics and chemistry, specifically within the sub-discipline of gas laws.
Etymology
The law is named after the Irish natural philosopher Robert Boyle (1627–1691), who first stated the law in 1662.
Definition
Boyle's Law states that the pressure (P) and volume (V) of a gas, at a constant temperature, are inversely proportional. This means that when the volume of a gas increases, its pressure decreases and vice versa, provided the temperature remains constant. Mathematically, this relationship is expressed as P*V = k, where k is a constant.
Related Terms
- Ideal Gas Law: An extension of Boyle's Law that also considers temperature and the number of gas particles.
- Charles' Law: Another gas law, which states that volume and temperature are directly proportional at constant pressure.
- Avogadro's Law: A gas law stating that equal volumes of all gases, at the same temperature and pressure, contain the same number of molecules.
Applications
Boyle's Law has numerous applications in real-world scenarios, including in the fields of respiratory physiology, scuba diving, and engineering. For example, it helps explain how our lungs expand and contract during breathing and how the pressure changes with depth under water.
See Also
External links
- Medical encyclopedia article on Boyle's law
- Wikipedia's article - Boyle's law
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