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Boyle's law
Boyle's law states that for a fixed amount of gas at constant temperature, pressure and volume are inversely proportional, so their product stays the same. Double the pressure and the gas takes up half the space. Robert Boyle published the law in 1662 after experiments with air pressure. In France it is often called Mariotte's law, after the physicist Edme Mariotte, who independently arrived at it.
Gas molecules constantly bump into the container walls and create pressure. Squeezing the gas into a smaller space makes these impacts more frequent, so the pressure rises in proportion as the volume falls.
It is one of the first quantitative laws about gases and a foundation of later kinetic theory. It explains everyday things like how a syringe, a bicycle pump or a diving lung behaves when squeezed.
Boyle's law is one of the gas laws that were later combined into the ideal gas law, which links pressure, volume, temperature and amount of gas.
In France the law is commonly called Mariotte's law, reflecting Edme Mariotte's independent work on it.
From Wikipedia, the free encyclopedia · text CC BY-SA 4.0
Illustrative photo · Reginaprice2013, CC BY-SA 3.0, via Wikimedia Commons
