BOYLE’S LAW
The relationship between volume and pressure of a gas was first started by Robert Boyle in 1662.
Boyle’s law states that the volume of a given mass of gas is inversely proportional to its pressure, provided that the temperature remains constant.
According to Boyle’s law, volume of a gas increases as the pressure decreases and vice versa.
This relationship is independent of the nature of the gas and it can be expressed mathematically as:
\(V ∝ \frac{1}{P} \\ ∴ V = \frac{k}{p} \)
or \(PV = k\)
Where V = Volume at pressure P
K = A mathematical constant
For a given mass of a gas, the product of its pressure and its volume is always a constant. If the pressure of a given mass of gas increases, its volume will decrease by a similar proportion and vice versa, as long as the temperature remain constant. This relationship can also be expressed mathematically as:
\(P_1 V_1 = P_2 V_2 \)
Where V1 = Volume at pressure P1
V2 = Volume at pressure P2
Boyle’s law can still be re-stated as: ‘The pressure of a given mass of gas is inversely proportional to its volume, provided the temperature remains constant.
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