Class 11 Physics Ch 13

 Kinetic Theory of Gases Class 11 Physics Ch 13 Notes 

Kinetic Theory of Gases Class 11 Doctor with Gas tubes

Class 11th Physics Solutions Notes, s Quick Revision notes pdf download, Online YouTube classes notes, chapter summary most important Points Notes, Physics wallah alakh Pandey pdf notes Kinetic Theory CBSE Class 1Ith Physics Notes

 CBSE NCERT Class 11th Physics Notes Cover a Wide Range of Important Topics and Concepts, including Work, Energy, and Power, Thermal Properties of Matter, Rotational Motion, Thermodynamics, Kinetic Theory, Gravitation, and Laws of Motion, and Much More.

CBSE Class 11 Chapter-wise Physics Notes

Class 11 physics Chapter 13 Kinetic Theory of Gases is an important study material for the Students who are presently studying in CBSE 11th standard. 

Gases have a minimal molecular interaction force. They have no shape or size and can be contained in any shape or size receptacle. As a result, gases expand forever and uniformly to cover the available space. Because gases are composed of atomic particles, numerous scientists, including Boyle and Newton, attempted to explain the behavior of gases.
However, Maxwell and Boltzmann discovered the true theory in the nineteenth century. In this chapter, we will look at several aspects of kinetic theory.

Key Notes for CBSE NCERT based Class 11th Physics

 The NCERT Results for Class 11 physics are matter experts according to the latest CBSE Syllabus 2023-24 and its marking schemes. Kinetic Theory of Gases  Physics Class 12 NCERT PDF can come easy to understand  while preparing notes and during  different Exams. Download Class 11 physics Chapter 
13 Notes from the link attached below at free or no cost.  


CBSE Class 11 Physics Chapter 13 Notes Kinetic Theory of Gases  

Kinetic Theory:

 Kinetic theory explains the behaviour of gases based molecules.

on rapidly moving atoms or

Molecular nature of matter: Everything in this universe is made up of atoms.

Atom move around in a perpetual order attracting each other when they are little distance apart But if they are forced very close to each other then they repel. Dalton's atomic theory: This theory proves that matter is made up of molecules which in turn are made up of atoms

Gay Lussac's law:

 when gases combine chemically to yield another gas, their volumes small integers.

• Avogadro's law: 

Equal volumes of all gases at equal temperature and pressure have the same number of molecules.

• Conclusion: - All these laws proved the molecular nature of goes

Behaviour of Gases: Gases at low pressures and high temperatures much above than

PV=KT (1)

This is the universal relation which is satisfied by all gases where P. V. T are pressure, volume and

temperature respectively and K is the constant 

• Conclusions. This relation is satisfied by all gases at low pressure and high temperature.

Avogadro's hypothesis from equation of gas: Avogadro's hypothesis states that equal volumes of all gases Therefore at equal temperature and pressure have the same number of molecules. • Avogadra number is denoted by N..

N. 6.02x102 It is universal value

• Experimentally it has been found that the mass of 22.4 litres of any gas is equal to molecular weight in grams at standard temperature and pressure

K-Boltzmann Constant and its value never change.

Perfect Gas Equation: Perfect gas equation is given by


• Where P.V are pressure, volume, T = absolute temperature, u= number of moles and R= universal gas constant. (R= 8.314Jmol 'K')

Ideal Gas: A gas that satisfies the perfect gas equation exactly at all pressures and temperatures
No real gas is truly ideal. A gas which is ideal is known as real gat Real gases deviation from ideal gas

• Real gases approach the ideal gas behaviour for low pressures and high temperatures 

⚫Graph should be a straight line (parallel to x-axis) for ideal gas

⚫But in case of real gases graph approach ideal gas behaviour

⚫This means it has constant value at all temperature and all

Real gases approach ideal gas behaviour at low pressures and high temperatures

400 P(at)

Deduction of Boyle's law and Charles law from perfect gas equation: 1 Boyle's law: According to Boyle low, at a constant temperature, pressure. of a given mass of gas varies inversely with volume. tody deduction of Boyle's law and Charles low from perfect gas equation: 

Volume V

1. Boyle's low:- According to Boyle's low, at a constant temperature, pressure

Pressure P

Dalton's Law of partial pressures:

 Dolton's law of partial pressure states that the total pressure of a mixture of ideal gases is the sum of partial pressures,

P=PL P₂+

To show how perfect gas equation concludes Dalton's law of partial pressure:-

By perfect gas equation PV = URTAs there are mixture of gases therefore use on

Charles's law for a fixed pressure, volume of a gas is

PV = (H)RT


Kinetic Theory of an Ideal Gas:

• Molecules of gas are in incessant randum motion, colliding against one another and with the walls of the container

• All collisions are elastic. • Total Kinetic energy is conserved.

Total momentum is conserved

In case of an elastic collision total Kinetic energy and momentum before calling is equal to the total Kinetic energy and momentum after collision

Pressure of an ideal gas: P(1/3)mm v

where, P = pressure

n=no. of molecules per unit V average of v

Law of Equipartition of energy: Degrees of Freedom • Degrees of Freedom can be defined as independent displacements or rotations that specify the dust orientation of a body or system.

A molecule free to move in space needs three coordinates to specify its location.

Categories of Degrees of Freedom:

1) Translational degree of freedom: Translation means motion of the body as a whale from one paint to

A molecule which is free to move in space and so it will need 3 coordinates (x, y, z) to specify its location. Therefore it has 3 degrees of freedom.

⚫ A molecule which is free to move in a plane which is 2 dimensional and so it needs 2 coordinates to specify its location. Therefore it has 2 degrees of freedom. 

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