What is Boyle’s Law?
It is one of the chemistry rules that govern how gases behave. A gas occupies less space while it is under pressure; the greater the pressure, the smaller the volume. The image added below shows how the increase in pressure decreases the volume of the gas.
It explains the link between a gas’s volume and pressure at a fixed temperature. It states that if the temperature of a mass is constant, the pressure of a given mass is inversely proportional to the volume of the given mass. It is also called a pressure-volume relationship.
P ∝ 1/V (at constant temperature (T))
PV = k where ‘k’ represents the Boyle’s constant)
PV = constant
If P1 , V1 be the initial pressure and volume of the given sample gas and P2 , V2 be the final pressure and volume of the given sample gas, then we can write as:
P1V1 = P2V2
Another way of defining Boyle’s Law, states that if the temperature of a mass is constant, the product of the pressure and volume of the given mass of a gas is constant.
Boyle’s Law
The English chemist Robert Boyle (1627–1691), widely regarded as one of the pioneers of the modern experimental science of chemistry, is commonly credited with this development. He found that increasing the pressure of a sample of contained gas by two times while holding its temperature constant reduced the gas volume by half. According to Boyle’s law, a gas’s volume changes inversely with pressure when the temperature is held constant. This is an illustration of an inverted relationship. The second variable drops when one variable rises in value.