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Boyle’s law is significant because it explains how gases behave. It proves beyond a shadow of a doubt that gas pressure and volume are inversely proportional. When you apply pressure on a gas, the volume shrinks and the pressure rises.
This is accompanied by an increase in the pressure exerted by the air on the balloon, as a consequence of Boyle’s law. As the balloon is squeezed further, the increasing pressure eventually pops it.
A balloon is a good example of Boyle’s law in action. The balloon is inflated by blowing air into it; the pressure of the air pulls on the rubber, causing the balloon to expand. When one end of the balloon is compressed, the pressure within rises, causing the un-squeezed section of the balloon to expand outward.
Boyle’s law. It can be observed that a straight line is obtained when the pressure exerted by the gas (P) is taken on the Y-axis and the inverse of the volume occupied by the gas (1/V) is taken on the X-axis.
Boyle’s law was put forward by the Anglo-Irish chemist Robert Boyle in the year 1662. For a gas, the relationship between volume and pressure (at constant mass and temperature) can be expressed mathematically as follows. Where P is the pressure exerted by the gas and V is the volume occupied by it.
Boyle’s law is a gas law which states that the pressure exerted by a gas (of a given mass, kept at a constant temperature) is inversely proportional to the volume occupied by it . In other words, the pressure and volume of a gas are inversely proportional to each other as long as the temperature and the quantity of gas are kept constant.