“Kinetic Theory Of Gases Class 11 Physics One Shot 🔥 | NCERT + Derivations | Physics Chapter 12”

Описание: “Kinetic Theory Of Gases Class 11 Physics One Shot 🔥 | NCERT + Derivations | Physics Chapter 12”
telegram channel: https//t.me/Physiconyourtips

Confused with Kinetic Theory of Gases – Class 11 Physics Chapter 13? 😵‍💫
This One Shot Power Revision by Vinod Kumar Behl Sir covers the entire NCERT chapter + all important derivations in the most exam-oriented & conceptual way 🔥

Perfect for Class 11 CBSE, NEET, JEE & school exams.

📌 In This One Shot, You Will Learn:

✅ Assumptions of Kinetic Theory of Gases
✅ Molecular Interpretation of Pressure
✅ Kinetic Energy & Temperature Relation
✅ RMS Speed, Average Speed & Most Probable Speed
✅ Derivation of PV = (1/3) mNv²
✅ Relation between KE and Temperature
✅ Degrees of Freedom
✅ Law of Equipartition of Energy
✅ Specific Heat Capacities (Cv & Cp)
✅ Mean Free Path
✅ Important NCERT derivations & PYQ concepts

🎯 Why Watch This Video?

• Complete chapter in one shot
• NCERT-focused explanations
• All important derivations covered
• Best for last-minute revision ⏱
• Ideal for Boards + NEET + JEE Foundation

📘 Chapter Covered:
Kinetic Theory of Gases – Class 11 Physics Chapter 13 (NCERT)


🎯 Who Should Watch?
Class 11 students preparing for Final Exams
Students revising NCERT Physics Chapter 13
Learners preparing for JEE/NEET foundation
Anyone wanting a crystal-clear conceptual understanding


👨‍🏫 Educator: Vinod Kumar Behl
📚 Physics for CBSE | NEET | JEE | CUET

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Gas Laws:
• Boyle's Law (3:22): States that at constant temperature, pressure is inversely proportional to volume (P ∝ 1/V), leading to PV = constant.
• Charles's Law (5:34): States that at constant pressure, volume is directly proportional to temperature (V ∝ T), leading to V/T = constant.
• Gay-Lussac's Law (8:55): States that at constant volume, pressure is directly proportional to temperature (P ∝ T), leading to P/T = constant.
• Perfect Gas Equation (11:01): Derives PV = nRT, where R is the universal gas constant (11:16), and introduces the relationship with Boltzmann constant (14:44) and Avogadro's number (13:47).
• Ideal Gas (16:05): Defines an ideal gas as one that follows PV = nRT at all temperatures and pressures, with assumptions like negligible molecular size and no intermolecular forces (16:21). It also discusses how real gases deviate from ideal gas behavior (17:51).
• Assumptions of Kinetic Theory of Gases (19:25): The video outlines eight main assumptions, including that gases consist of rigid, elastic molecules, molecules are in random motion, collisions are perfectly elastic, there are no intermolecular forces, and internal energy is purely kinetic.
• Molecular Interpretation of Pressure / Derivation of PV = (1/3) mNv² (24:36): This section provides a detailed derivation of the pressure exerted by a gas on the walls of a container, leading to the formula P = (1/3) ρv² where ρ is density (34:16).
• Relation between Kinetic Energy and Temperature (37:56): The video derives the relationship between the kinetic energy of gas molecules and temperature, showing that kinetic energy per mole is (3/2)RT and for one molecule is (3/2)kT (39:11).


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