Kinetic Theory Of Gases Chapter 12 Class 11 Physics Important Questions Handwritten Notes

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Kinetic Theory also describe Properties such as Temperature, Thermal conductivity.

About Kinetic Theory Of Gases👇

• Kinetic Theory of Gases describes how gases behave by assuming that molecules in gases are loosely packed due to huge intermolecular spaces

Kinetic Theory of Gases explains random movement of molecules in gases.

Molecular Nature of Matter

Atoms are Tiny Particles that move around in a constant order attracting one another when they are close enough. When they are forced to be very close to each other however they repel each other.

PDF -1 Important Questions Kinetic Theory of Gases Chapter 12 Class 11 Physics

• According to Avogadro’s law all gases have same number of Molecules in Equal Volumes at the same temperature & Pressure.

Perfect Gas Equation

• A Perfect gas equation is given by PV = nRT where P is Pressure ,V is Volume , T is absolute Temperature, n is no of Moles & R is Universal gas Constant.

• This equation describes how gas behaves in a Specific Condition.

• If a gas fulfills this equation it is referred to as a Perfect gas or Ideal gas.

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Ideal Gas

At all Pressure & Temperature a gas that exactly fulfills the perfect gas equation.

Concept of an ideal gas is purely theoretical.

There is no such thing as an ideal gas term real gas refers to a gas that is ideal.

For low Pressure & High Temperature real gas approach ideal gas behaviour.

Kinetic Theory of an ideal Gas

• Gas Molecules are in constant state of Random Motion interacting with one another and Container’s Wall.

• Every Collision is Elastic.

• Kinetic Energy is conserved in total.

• Total momentum of system is conserved.

• Total Kinetic & Momentum before collision is identical to the total kinetic energy & Momentum After Collision in event of an elastic Collision.

Kinetic Interpretation Of Temperature

A Molecule’s Average kinetic energy is proportional to absolute Temperature of gas. It is unaffected by Ideal gas ‘s pressure., Volume or Nature.

law Of Equipartition Of Energy

For any dynamical system Total energy is distributed Equally among all molecules per degree of Freedom i. e 1/2 k_B T.

•Each Translational Degree of freedom Contributes 1/2 K_B.

• Each Degree of Rotational freedom provides 1/2 K_B.

• Each Degree of Vibrational freedom Contributes two times of 1/2 K_B.

Mean Free Path

• Average distance between two successive collision is known as mean free path.

• With in the gas many molecules are randomly moving & Interacting with one another.

• Mean free path is distance that a gas molecule can travel without interacting.

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