Equilibrium Chemistry Class 11 | Chapter 7 Chemical Equilibrium One Shot | CBSE NEET JEE

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0:00 Introduction
0:50 Equilibrium
3:39 Dynamic Equilibrium
9:16 Dynamic Physical Equilibrium
10:16 Solid Liquid Equilibrium
12:01 Liquid-Vapour Equilibrium
12:27 Solid-Vapour Equilibrium
14:43 Dissolution of Solid in Liquids
16:38 Dissolution of Gases in Liquids
19:25 Characteristics of Physical Equilibrium
20:02 Chemical Equilibrium
25:33 Chemical Equilibrium Example
26:33 Reversible reactions:Examples
27:33 Depiction of Equilibrium
29:35 Chemical Equilibrium:Characteristics
31:44 Law of Mass Action
33:03 Equilibrium Constant
36:02 Law of chemical equilibrium
39:08 Steps for writing equilibrium constant
43:29 Equilibrium constant in Gaseous System
51:44 Hetergeneous 7 Homogeneous Mixture
52:40 Characteristics of Equilibrium constant
1:02:13 Applications of Equilibrium constant
1:05:10 Predict the direction of the reaction
1:07:27 Example on predicting the direction of the reaction
1:10:31 Example 1 on calculating equilibrium constant
1:17:10 Example 2 on calculating equilibrium constant
1:21:43 K,Q And G relationship
1:26:38 Example : K,Q And G relationship
1:27:32 Factors affecting equilibrium
1:30:07 Le Chatelier’s Principle
1:31:43 Effect of concentration change
1:34:24 Effect of change of pressure
1:38:00 Effect of change of volume
1:40:34 Effect of temperature change
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In this video we will cover all concepts and some numerical problems:-
7.Example 1:- For the following equilibrium, Kc = 6.3 × 1014 at 1000 K ,
NO (g) + O3 (g) ⇌NO2 Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is Kc ,for the reverse reaction?
10.For the equilibrium,2NOCl(g) ⇌ 2NO(g) + Cl2 (g)
the value of the equilibrium constant, Kc is 3.75 × 10–6 at 1069 K. Calculate the Kp for the reaction at this temperature?
13. The value of Kc for the reaction 2A ⇌ B + C is 2 × 10–3. At a given time,the composition of reaction mixture is [A] = [B] = [C] = 3 × 10–4 M. In which direction the reaction will proceed?
14.13.8g of N2O4 was placed in a 1L reaction vessel at 400K and allowed to attain equilibrium N2O4(g) ⇌ 2NO2 (g)
The total pressure at equilbrium was found to be 9.15 bar. Calculate Kc,Kp and partial pressure at equilibrium.
15.One mole of H2O and one mole of CO are taken in 10 L vessel and heated to 725 K. At equilibrium 40% of water (by mass) reacts with CO according to the equation, H2O (g) + CO (g) ⇌ H2(g) + CO2(g)
Calculate the equilibrium constant for the reaction?
17.Hydrolysis of sucrose gives, Sucrose + H2O ⇌ Glucose + Fructose Equilibrium constant Kc for the reaction
is 2 ×1013 Calculate ∆G0 at 300K.
24.Example:-Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:
CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g)
(a) Write as expression for Kp for the above reaction.
(b) How will the values of Kp
and composition of equilibrium mixture be affected by
(i) increasing the pressure
(ii) increasing the temperature
(iii) using a catalyst ?

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