Where Discovery Begins

# States of Matter – Class 11 Chemistry | Chapter 5 | One Shot

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Timestamps:
0:00 Introduction
4:38 Intermolecular forces
8:26 van der Waals Forces
9:12 Polar Vs non-Polar molecules
12:44 London Forces
19:47 Dipole-Dipole force
24:40 Dipole-Induced Dipole force
29:35 Gaseous States
30:07 Gas Laws
31:04 Gas Properties
33:56 Boyle’s Law
35:29 Isotherms
36:51 Boyle’s Law:Conclusion
37:45 Ex 1
38:51Charles’ Law
40:13 Charles Law:Graph
44:11Ex2
45:33 Gay Lussac’s Law
48:05 Gay Lussac’s Law:Graph
48:31 Avogardo’s law
50:36 Ideal Gas
52:16 Ideal gas Equation
54:24 Value of R
55:26 Ex3
57:24 Density & Molar Mass
59:03 Dalton’s Law of Partial Pressures
1:00:46 Mole fraction
1:03:18 Ex4
1:04:54 Kinetic theory of gases
1:07:48 KMT Postulates
1:11:17 Real Gas:Behaviour
1:13:55 Deviate:Real Gas
1:16:14 Real GAs Equation
1:19:42 Compressibility Factor

There are 3 different states of matter, namely solid, liquid, gas.The particles, or the atoms, ions and molecules, are packed together closely.They have a fixed volume, if the pressure and temperature are kept unchanged.The particles in a gaseous state have enough
kinetic energy in it so as to render the molecular forces to zero.The gas laws(Boyle’s law,Charles’Law,Avogardo’s law,Dalton’s law of partial pressures) were developed at the end of the 18th century, when scientists began to realize that relationships between pressure, volume and temperature of a sample of gas.The Ideal Gas Law states that under the same temperature, pressure and volume all gases contain the same number of molecules.At low temperatures or high pressures, real gases deviate significantly from ideal gas behavior.In this video we will cover:-
1.Introduction to solids,liquids and gaseous state of matter.
2.What are intermolecular Forces?
3.What are van der waals forces?
4.What are polar and non-polar molecules?
5.What are London forces?
6.What is dipole-dipole force?
7.What is dipole-induced dipole force?
8.Understanding Gaseous state.
9.What are different Gas laws?
10.Different gas properties.
11.Explanation of Boyle’s Law.
12.Boyle’s law Graphs(Isotherms)
13.What is the Conclusion of Boyle’s law?
14.A vessel of 120 mL capacity contains a certain amount of gas at 35 °C and 1.2bar pressure. The gas is transferred to another vessel of volume 180 mL at 35°C. What would be its pressure?
15.Explanation of Charles’ law.
16.Graphical representation of Charle’s law.
17.On a ship sailing in pacific ocean where temperature is 23.4 °C , a balloon is filled with 2 L air. What will be the volume of the balloon when the ship reaches Indian ocean, where temperature is 26.1°C ?
18.Explanation on Gay-Lussac’s law.
19.Graphical representation of Gay Lussac’s Law.
21.What are ideal gases?
22.What is ideal gas equation?
23.Ideal Gas Equation: Value of R
24.At 25°C and 760 mm of Hg pressure a gas occupies 600 mL volume. What will be its pressure at a height where
temperature is 10°C and volume of the gas is 640 mL.
25.Density & Molar mass of a Gaseous Substance.
26.What is Dalton’s Law of partial pressures?
27.Partial pressures in terms of mole fraction.
28.Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm3 at 27°C. R = 0.083 bar dm3 K–1 mol–1.
29.What is Kinetic theory of gases?
30.Postulates of Kinetic theory of Gases.
31.Behaviour of real gases?
32.Why do gases deviate from the ideal behaviour?
33. Explaining about Real Gas Equation.
34.What is compressibility factor?
35.Compressibility factor (Negative & Positive)

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