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Are you struggling to solve Equilibrium exercise problems from the NCERT textbook for Class 11? Look no further than our comprehensive solution guide, "Class 11 Unit 7 Equilibrium Exercise Solution 7.1 to 7.10 NCERT Solution 2023," available on YouTube.
This educational video is designed specifically to help students of Class 11 understand and solve Equilibrium exercise problems. Our experienced tutor begins by introducing the importance of Equilibrium in chemistry, and then proceeds to explain concepts such as Le Chatelier's Principle, Equilibrium Constants, and Equilibrium Expressions.
Our tutor then takes up each problem from the NCERT textbook and provides step-by-step solutions, ensuring that students can understand and follow along with ease. Throughout the video, our tutor emphasizes the importance of understanding the concepts underlying each problem, rather than simply memorizing the solutions.
Whether you're struggling with NCERT solutions or simply looking to improve your knowledge of Equilibrium, this video is an invaluable resource for students seeking to enhance their understanding and problem-solving skills in chemistry.
So, if you're a Class 11 student looking to excel in
Equilibrium exercises, make sure to check out our video, "Class 11 Unit 7
Equilibrium Exercise Solution 7.1 to 7.10 NCERT Solution 2023," and start
solving problems with confidence!
7.1 A liquid is in equilibrium with its vapour in a sealed
container at a fixed temperature. The volume of the container is suddenly
increased.
a) What is the initial effect of the change on vapour
pressure?
b) How do rates of evaporation and condensation change
initially?
c) What happens when equilibrium is restored finally and
what will be the final vapour pressure?
7.2 What is Kc for the following equilibrium when the
equilibrium concentration of each substance is: [SO2] = 0.60M, [O2] = 0.82M and
[SO3] = 1.90M ?
2SO2(g) + O2(g) ⇌ 2SO3(g)
7.3 At a certain temperature and total pressure of 105Pa, iodine
vapour contains 40% by volume of I atoms
I2(g) ⇌ 2I(g)
Calculate Kp for the equilibrium.
7.4 Write the expression for the equilibrium constant, Kc
for each of the following reactions:
(i) 2NOCl(g) ⇌ 2NO(g) + Cl2(g)
(ii) 2Cu(NO3)2(s) ⇌ 2CuO(s) + 4NO2(g) + O2(g)
(iii) CH3COOC2H5(aq) + H2O(l) ⇌ CH3COOH(aq) + C2H5OH(aq)
(iv) Fe3+(aq) + 3OH–(aq) ⇌ Fe(OH)3(s)
(v) I2(s) + 5F2 ⇌ 2IF5
7.5 Find out the value of Kc for each of the following
equilibria from the value of Kp:
(i) 2NOCl(g) ⇌ 2NO(g) + Cl2(g); Kp = 1.8 × 10–2 at 500 K
(ii) CaCO3(s) ⇌ CaO(s) + CO2(g); Kp= 167 at 1073
K
7.6 For the following equilibrium, Kc= 6.3 × 1014 at 1000 K
NO(g) + O3(g) ⇌ NO2(g) + O2(g)
Both the forward and reverse reactions in the equilibrium
are elementary bimolecular reactions. What is Kc, for the reverse reaction?
7.7 Explain why pure liquids and solids can be ignored while
writing the equilibrium constant expression?
7.8 Reaction between N2 and O2 takes place as follows:
2N2(g) + O2(g) ⇌ 2N2O(g)
If a mixture of 0.482 mol N2 and 0.933 mol of O2 is placed
in a 10 L reaction vessel and allowed to form N2O at a temperature for which
Kc= 2.0 × 10–37, determine the composition of equilibrium mixture.
7.9 Nitric oxide reacts with Br2 and gives nitrosyl bromide
as per reaction given below:
2NO(g) + Br2(g) ⇌ 2NOBr(g)
When 0.087 mol of NO and 0.0437 mol of Br2 are mixed in a
closed container at constant temperature, 0.0518 mol of NOBr is obtained at
equilibrium. Calculate equilibrium amount of NO and Br2.
7.10 At 450K, Kp = 2.0 × 1010/bar for the given reaction at
equilibrium.
2SO2(g) + O2(g) ⇌ 2SO3(g)
What is Kc at this temperature?