Class 11 Unit 7 Equilibrium Exercise Solution 7.1 to 7.10 NCERT Solution 2023

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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?

THERMODYNAMICS Exercise Solution 6.1 to 6.5, Class 11 Chemistry Chapter 6

 

6.1 Choose the correct answer. A thermodynamic state function is a quantity 

(i) used to determine heat changes

(ii) whose value is independent of path

(iii) used to determine pressure volume work

(iv) whose value depends on temperature only.

6.2 For the process to occur under adiabatic conditions, the correct condition is:

(i) ∆T = 0

(ii) ∆p = 0

(iii) q = 0

(iv) w = 0

6.3 The enthalpies of all elements in their standard states are:

(i) unity

(ii) zero

(iii)  0

(iv) different for each element

6.4 ∆U° of combustion of methane is – X kJ mol^–1. The value of ∆H° is

(i) = ∆U°

(ii)  ∆U°

(iii)  ∆U°

(iv) = 0

6.5 The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, –890.3 kJ mol^–1 –393.5 kJ mol^–1, and –285.8 kJ mol^–1 respectively. Enthalpy of formation of CH_4(g) will be

(i) –74.8 kJ mol^–1 

(ii) –52.27 kJ mol^–1

(iii) +74.8 kJ mol^–1 

(iv) +52.26 kJ mol^–1.

Class 11 Chemistry Chapter 1 Some Basic Concept of Chemistry Exercise Solution Question 1.11

 

Class 11 Chemistry Chapter 1 Some Basic Concept of Chemistry Exercise Solution Question 1.11

Chemistry Class 11 Unit 1 Some Basic Concept of Chemistry, Missing Question's Exercise Solution

 

Hi guys,This Dr. Nileshkumar Vala from My Smart Class and in this video I am going to teach you all about Chemistry Class 11 Unit 1 Some Basic Concept of Chemistry, Missing Question's Solution.

chemistry class 11 chapter 1 exercise questions and answers

Hope you like it :) Thanks For Watching :) 

Time Stamp of Numerical is given below in the description.

00:36 Question 1.14: What is the SI unit of mass? How is it defined?

01:04 Question 1.15: Match the following prefixes with their multiples:

01:24 Question 1.16: What do you mean by significant figures?

02:52 Question 1.19:How many significant figures are present in the following?(i) 0.0025(ii) 208(iii) 5005(iv) 126,000(v) 500.0(vi) 2.0034

04:02 Question 1.20:Round up the following upto three significant figures:(i) 34.216(ii) 10.4107(iii) 0.04597(iv) 2808

05:54 Question 1.23: In a reactionA + B2  AB2Identify the limiting reagent, if any, in the following reaction mixtures.(i) 300 atoms of A + 200 molecules of B(ii) 2 mol A + 3 mol B(iii) 100 atoms of A + 100 molecules of B(iv) 5 mol A + 2.5 mol B(v) 2.5 mol A + 5 mol B

09:10 Question 1.24: Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation:

N2(g) + H2(g)  2NH3(g)(i) Calculate the mass of ammonia produced if 2.00 × 103 g dinitrogen reacts with 1.00 ×103 g of dihydrogen.(ii) Will any of the two reactants remain unreacted?(iii) If yes, which one and what would be its mass?

13:59 Question 1.25: How are 0.50 mol Na2CO3 and 0.50 M Na2CO3 different?

15:07 Question 1.26:If 10 volumes of dihydrogen gas reacts with five volumes of dioxygen gas, howmany volumes of water vapour would be produced?

16:12 Question 1.27:Convert the following into basic units:(i) 28.7 pm(ii) 15.15 pm(iii) 25365 mg

18:26 Question 1.28:Which one of the following will have the largest number of atoms?(i) 1 g Au (s)(ii) 1 g Na (s)(iii) 1 g Li (s)(iv) 1 g of Cl2(g)

19:09 Question 1.30: What will be the mass of one 12C atom in g?

19:35 Question 1.31:How many significant figures should be present in the answer of the following calculations?

20:54 Question 1.33: Calculate the number of atoms in each of the following 

(i) 52 moles of Ar 

(ii) 52 u of He 

(iii) 52 g of He.

Class 11 Chemistry Chapter 1 Some Basic Concept of Chemistry Full Exercise Solution with explanation

 

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Std 11, Chemistry, unit 1, full exercise solution

Class 11 Chemistry Chapter 1 Some Basic Concept of Chemistry Full Exercise Solution with explanation

1.1 Calculate the molar mass of the following:

(i) H2O (ii) CO2 (iii) CH4

1.2 Calculate the mass per cent of different elements present in sodium sulphate(Na2SO4).

1.3 Determine the empirical formula of an oxide of iron, which has 69.9% iron and 30.1% dioxygen by mass.

1.4 Calculate the amount of carbon dioxide that could be produced when

(i) 1 mole of carbon is burnt in air.

(ii) 1 mole of carbon is burnt in 16 g of dioxygen.

(iii) 2 moles of carbon are burnt in 16 g of dioxygen.

1.5 Calculate the mass of sodium acetate (CH3COONa) required to make 500 mL of

0.375 molar aqueous solution. Molar mass of sodium acetate is 82.0245 g mol–

1..6 Calculate the concentration of nitric acid in moles per litre in a sample which has a density, 1.41 g mL–1 and the mass per cent of nitric acid in it being 69%.

1.7 How much copper can be obtained from 100 g of copper sulphate (CuSO4)?

1.8 Determine the molecular formula of an oxide of iron, in which the mass per cent of iron and oxygen are 69.9 and 30.1, respectively.

1.9 Calculate the atomic mass (average) of chlorine using the following data:

% Natural Abundance Molar Mass

1.10 In three moles of ethane (C2H6), calculate the following: (i) Number of moles of carbon atoms. (ii) Number of moles of hydrogen atoms. (iii) Number of molecules of ethane.

1.11 What is the concentration of sugar (C12H22O11) in mol L–1 if its 20 g are dissolved in enough water to make a final volume up to 2L?

1.12 If the density of methanol is 0.793 kg L–1, what is its volume needed for making 2.5 L of its 0.25 M solution?

1.13 Pressure is determined as force per unit area of the surface. The SI unit of

pressure, pascal is as shown below:

1Pa = 1N m–2

If mass of air at sea level is 1034 g cm–2, calculate the pressure in pascal.

1.14 What is the SI unit of mass? How is it defined?

1.15 Match the following prefixes with their multiples:

To watch solution of missing question, click on below button

1.17 A sample of drinking water was found to be severely contaminated with chloroform,

(i) Express this in per cent by mass.

(ii) Determine the molality of chloroform in the water sample.

1.18 Express the following in the scientific notation:

(i) 0.0048

(ii) 234,000

1.19 How many significant figures are present in the following?

(i) 0.0025

(ii) 208

(iii) 5005

(iv) 126,000

(v) 500.0

(vi) 2.0034

1.20 Round up the following upto three significant figures:

(i) 34.216

(ii) 10.4107

(iii) 0.04597

(iv) 2808

1.21 The following data are obtained when dinitrogen and dioxygen react together to

form different compounds:

Mass of dinitrogen Mass of dioxygen

(i) 14 g 16 g

(ii) 14 g 32 g

(a) Which law of chemical combination is obeyed by the above experimental data?

Give its statement.

(b) Fill in the blanks in the following conversions:

(i) 1 km = ...................... mm = ...................... pm

(iii) 1 mL = ...................... L = ...................... dm3

1.22 If the speed of light is 3.0 × 108 m s–1, calculate the distance covered by light in

2.00 ns.

Identify the limiting reagent, if any, in the following reaction mixtures.

(i) 300 atoms of A + 200 molecules of B

(ii) 2 mol A + 3 mol B

1.24 Dinitrogen and dihydrogen react with each other to produce ammonia according

to the following chemical equation:

(i) Calculate the mass of ammonia produced if 2.00 × 103 g dinitrogen reacts

with 1.00 ×103 g of dihydrogen.

1.26 If 10 volumes of dihydrogen gas reacts with five volumes of dioxygen gas, how

many volumes of water vapour would be produced?

1.27 Convert the following into basic units:

(i) 28.7 pm

1.28 Which one of the following will have the largest number of atoms?

(i) 1 g Au (s)

1.29 Calculate the molarity of a solution of ethanol in water, in which the mole fraction of

ethanol is 0.040

1.30 What will be the mass of one 12C atom in g?

1.31 How many significant figures should be present in the answer of the following

calculations?

1.32 Use the data given in the following table to calculate the molar mass of naturally

occuring argon isotopes:

1.33 Calculate the number of atoms in each of the following (i) 52 moles of Ar (ii)

52 u of He (iii) 52 g of He.

1.34 A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it

in oxygen gives 3.38 g carbon dioxide, 0.690 g of water and no other products. 

3 (s) + 2 HCl (aq) → CaCl2 (aq) + CO2(g) + H2O(l)

What mass of CaCO

3 is required to react completely with 25 mL of 0.75 M HCl?

1.36 Chlorine is prepared in the laboratory by treating manganese dioxide (MnO2) with

aqueous hydrochloric acid according to the reaction