Boyle’s law

Ideal gases are composed of rigid sphere molecules which are in random motion.  They can colloid with other molecules and wall of container. The collisions between molecules are completely elastic and due to this there is no loss of energy during collision. The average kinetic energy of molecules is directly proportional to temperature. All properties of ideal gas can be described by ideal gas equation given by;
PV = nRT

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Ideal gas law is a combination of ideal gas laws which give relation between variables of gases like pressure, number of moles of gas, temperature and volume. Let’s discuss one of the laws known as Boyle’s law.

In 1626, Robert Boyle purposed a relationship between the pressure (p) and the volume (V) of a confined gas held at a constant temperature and for a constant amount.

Let’s first define Boyle’s law. According to Boyle’s law, the product of the pressure and volume is nearly constant at constant temperature and number of moles of an ideal gas. See what is Boyle’s

Law Formula from the given definition, it would be;
P x V = constant (at constant T and n)
Or P  ? 1/V

Boyle’s law can be written for two different volume and pressure;
P1V1= k = P2V2
Or P1V1= P2V2

Boyle’s law graph can be shown in two ways; P v/s V (hyperbola) and P v/s 1/V (linear). The
graphical representation of Boyle’s law is follow;

This law can only apply on an ideal gas not on real gases. The pressure and volume do not show same relationship on the compression of real gas. However this law is good enough to calculate the pressure and volume of internal-combustion engines and steam engines.

Boyle’s Law can explain by using Boyle’s law demonstration.  Let’s take a gas cylinder and put a piston on that for applying pressure on gas.  Keep this cylinder in water bath to maintain constant temperature throughout the experiment.  At initial stage; pressure of gas is 1 atm and volume is 8 ml. As we doubled the pressure that is 1 x 2 atm=2 atm, volume of gas becomes half; 8/2=4 ml.  Again the same thing observed as we double pressure, volume of gas becomes half.

It proves that at constant temperature and constant amount of gas, the pressure of gas is inversely proportional to the volume of gas.  This is because, as pressure on gas increases, the intermolecular space between molecules decreases and they come closer to each other.

For example; in a balloon as the pressure around a balloon are increases, volume of balloon decrease and vice-versa.

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