Boyle’s Law is an ideal gas law that states the volume of an ideal gas is inversely proportional to the absolute pressure at the constant pressure. This law is applicable to the ideal gases only where only pressure and volume subject to change. In other words, the product of pressure or volume will remain constant at the fixed mass of ideal gas and at fixed temperature.

In simple words, Boyle’s Law is used to find the relationship between the pressure or volume of a gas. In most of the cases, pressure and volume had a direct relationship. If the volume increases then the pressure will go down and if pressure increases then the volume will go down. The equation for Boyle’s Law in chemistry could be written as:

\[\ P1 \times V1 = P2 \times V2 \]

Where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and the V2 is the final volume. Pressure is measured in atm units and the volume if given in liters. This does not matter generally which units are given for the volume or pressure but they should be the same at both ends. The other popular method to represent the Boyle’s Law is given below –

\[\ V \alpha \frac{1}{P} (f) \;or\; T = Constant \]

Where

P denotes pressure of the gas

V denotes volume of the gas

K is constant and holds units of force times and distance.

Where

P denotes pressure of the gas

V denotes volume of the gas

K is constant and holds units of force times and distance.

As soon as the temperature remains constant, the total amount of energy in the system will remain constant throughout the operations and value is present with alphabet k.