Boyle's Law
By
Muhammad Rizwan-971
Almas Haider-946
Hussnain Asghar-950
Muhammad Suleman bin -965
Muhammad Usman-985
Boyle’s Law

At constant temperature volume of a gas is
inversely proportional to the pressure.
Mathematically
V α 1/P
V= k/P
K = PV

Temperature is constant
Amount of gas is constant

Explanation:


At constant temperature, the product of pressure and volume of a
gas is always constant.
If P1 and V1 are initial pressure and volume and P2 and V2 are
final pressure and volume.
Then
P1V1 = k
P2V2 = k
P1V1 = P2V2
Hence prove
Experimental:
Graphical:

Pressure and Volume

The curve goes away from both axis. The isotherm
at 0oC is closer to the both axis but at 25oC goes
away from both axis.
Graphical

Pressure and 1/Volume

We get a straight line because pressure and
1/volume are directly proportional.
Graphical

Product of PV and Pressure

We get a straight line parallel to x-axis. This straight line
shows that “k” is a constant quantity.
Limitations:

The law hold good only at moderate
temperature and pressure.

At low Pressure.


The particles are father apart, so these
intermolecular forces are very weak, and this law
holds well.
At moderate to high temperature.

The particles move to fast for the weak
intermolecular forces to be attracted by them.
Limitation:

This law fails at high pressure and low
temperature.

At low temperature and high pressure.


The speed of the gas molecules decreases and
move closer together.
Boyle’s law is only applicable for ideal gas.

So, under the condition, a real gas will liquefy.
Observation:

At constant temperature, the greater the
force exerted on the trapped air, the
smaller the volume of a given amount of a
gas.
Application:

Boyle’s law observed in day-to-day life.

Spray , painting , drawing fluid into a syringe
pump up a bike tire.
This was a Brief discussion about
Boyle’s Law