NCERT Solutions for Class 11 Chemistry Equilibrium Part-1

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NCERT Solutions for Class 11 Chemistry Equilibrium Part-1 solutions are available in PDF format for free download. These ncert book chapter wise questions and answers are very helpful for CBSE board exam. CBSE recommends NCERT books and most of the questions in CBSE exam are asked from NCERT text books. Chemistry chapter wise Solutions for Class 11  and all the chapters can be downloaded from our website and myCBSEguide mobile app for free.

NCERT solutions for Class 11 Chemistry Download as PDF

NCERT Solutions for Class 11 Chemistry Equilibrium Part-1

NCERT Class 11 Chemistry Chapter wise Solutions

  • 1 – Some Basic Concepts of Chemistry
  • 2 – Structure of Atom
  • 3 – Classification of Elements and Periodicity in Properties
  • 4 – Chemical Bonding and Molecular Structure
  • 5 – States of Matter
  • 6 – Thermodynamics
  • 7 – Equilibrium
  • 8 – Redox Reactions
  • 9 – Hydrogen
  • 10 – The s-Block Elements
  • 11 – The p-Block Elements
  • 12 – Organic Chemistry – Some Basic Principles and Techniques
  • 13 – Hydrocarbons
  • 14 – Environmental Chemistry

NCERT Solutions for Class 11 Chemistry Equilibrium Part-1

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?

2. What is for the following equilibrium when the equilibrium concentration of each substance is: [ ]= 0.60 M, [ ] = 0.82 M and [ ] = 1.90 M ?
3. At a certain temperature and total pressure of 105 Pa, iodine vapour contains 40% by volume of I atoms Calculate for the equilibrium.

4. Write the expression for the equilibrium constant, Kc for each of the following reactions:

5. Find out the value of Kc for each of the following equilibria from the value of Kp:

6. For the following equilibrium,

Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is , for the reverse reaction?

7. Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression?

8. Reaction between takes place as follows:

If a mixture of 0.482 mol of and 0.933 mol of is placed in a 10 L reaction vessel and allowed to form at a temperature for which , determine the composition of equilibrium mixture.

9. Nitric oxide reacts with and gives nitrosyl bromide as per reaction given below:

When 0.087 mol of NO and 0.0437 mol of are mixed in a closed container at constant temperature, 0.0518 mol of NO Br is obtained at equilibrium. Calculate equilibrium amount of NO and .

10. At 450 K, bar for the given reaction at equilibrium.

What is at this temperature?

11. A sample of is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What is for the given equilibrium?

12. A mixture of 1.57 mol of , 1.92 mol of and 8.13 mol of is introduced into a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant, for the reaction

Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

13. The equilibrium constant expression for a gas reaction is,

Write the balanced chemical equation corresponding to this expression.

14. One mole of 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,

Calculate the equilibrium constant for the reaction.

15. At 700 K, equilibrium constant for the reaction

is 54.8. If 0.5 of is present at equilibrium at 700 K, what are the concentration of assuming that we initially started with and allowed it to reach equilibrium at 700 K?

16. What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M?

17. = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

18. Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:

(i) Write the concentration ratio (reaction quotient), , for this reaction (note: water is not in excess and is not a solvent in this reaction)

(ii) At 293 K, if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.

(iii) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after sometime. Has equilibrium been reached?

19. A sample of pure was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of was found to be . If value of is 8.3 × , what are the concentrations of at equilibrium?

20. One of the reactions that takes place in producing steel from iron ore is the reduction of iron (II) oxide by carbon monoxide to give iron metal and .

FeO (s) + CO (g) Fe (s) + (g); Kp= 0.265 at 1050 K.

What are the equilibrium partial pressures of CO and at 1050 K if the initial partial pressures are: = 1.4 atm and = 0.80 atm?

21. Equilibrium constant, for the reaction

at 500 K is 0.061.

At a particular time, the analysis shows that composition of the reaction mixture is 3.0 , 2.0 and 0.5 mol . Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

22. Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium:

for which Kc= 32 at 500 K. If initially pure BrCl is present at a concentration of , what is its molar concentration in the mixture at equilibrium?

23. At 1127 K and 1 atm pressure, a gaseous mixture of CO and in equilibrium with solid carbon has 90.55% CO by mass . Calculate for this reaction at the above temperature.

24. Calculate a) ΔG°and b) the equilibrium constant for the formation of from NO and at 298 K Where = 52.0 kJ/mol

= 87.0 kJ/mol

= 0 kJ/mol

25. Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?




NCERT Solutions for Class 11 Chemistry Chapter 7 Equilibrium

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