Exam-Style Online Test | Class 11 Chemistry: Equilibrium

Class 11 Chemistry — Chapter 7: Equilibrium Online Test

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Class 11 Chemistry: Equilibrium Online Test (Paper 1)

Welcome to Paper 1! This is your foundation to build confidence and get you ready to tackle the challenges ahead.

  • Total Questions: 20
  • Time Allotted: 30 minutes
  • Passing Score: 40%
  • Randomization: No
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

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1 / 20

1. In qualitative inorganic analysis, group IV cations are precipitated in ammoniacal medium because

2 / 20

2. If the solubility of (AgCl) is , the value is

3 / 20

3. When in a basic buffer, the pH equals

4 / 20

4. The hydrolysis constant is defined as

5 / 20

5. The pH of a (0.1,M) solution of is

6 / 20

6. The (pH) of a (0.2,M) solution is

7 / 20

7. The pH of a solution is defined as

8 / 20

8. According to Ostwald’s law, the degree of ionization is related to

9 / 20

9. For a weak base solution where , the hydroxide ion concentration is

10 / 20

10. The ionization constant of an acid is a measure of its

11 / 20

11. In the reaction , the Brønsted–Lowry base is

12 / 20

12. When the concentration of a reactant is increased in a system at equilibrium, the equilibrium

13 / 20

13. The main difference between and is that

14 / 20

14. For a general reaction , the expression for is

15 / 20

15. For at fixed (T), raising the external pressure of an inert gas at constant volume changes the extent of decomposition

16 / 20

16. For at a temperature where , starting with stoichiometric at 1 atm, the equilibrium extent toward is

17 / 20

17. The reaction has at 500 K. If initially is high and are low, the reaction will

18 / 20

18. For the equilibrium , the equilibrium constant expression is

19 / 20

19. For a heterogeneous equilibrium such as , the equilibrium constant is expressed as:

20 / 20

20. For at , . If initially and , the reaction will:

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Class 11 Chemistry: Equilibrium Online Test (Paper 2)

Welcome to Paper 2! You’ve mastered the basics, and now it’s time to test your understanding with a more challenging set of questions.

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  • Total Questions: 30
  • Time Allotted: 45 minutes
  • Passing Score: 50%
  • Randomization: Yes
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

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1 / 30

1. Which pair correctly represents a Lewis acid–base adduct?

2 / 30

2. For , the value of at temperature (T) is governed by

3 / 30

3. According to the Lewis concept, a Lewis acid is defined as a species that

4 / 30

4. If for a given reaction mixture, the reaction will

5 / 30

5. Which statement about catalysts relates correctly to the definition of equilibrium?

6 / 30

6. In dissolution equilibrium of a solid in a liquid (at fixed (T)), which action increases the amount of undissolved solid without changing solubility?

7 / 30

7. The pH of a (0.01,M) solution of (HCl) is

8 / 30

8. The optimum temperature for the Contact process is around

9 / 30

9. When temperature increases, the numerical value of relative to :

10 / 30

10. For a heterogeneous equilibrium such as , the equilibrium constant is expressed as:

11 / 30

11. If for the reaction at 300 K, the value of is

12 / 30

12. For a salt of a weak base and strong acid, the expression for pH is

13 / 30

13. For a system at constant (T) and (P), a spontaneous process always has

14 / 30

14. For , with and initial , equilibrium is

15 / 30

15. When equilibrium is reached in the reaction , what best explains macroscopic constancy?

16 / 30

16. If an inert gas is added at constant pressure, the equilibrium shifts

17 / 30

17. If , the reaction will proceed

18 / 30

18. In the Contact process, the catalyst used to oxidize is

19 / 30

19. In the reaction , the conjugate base of the acid (HCl) is

20 / 30

20. In the equilibrium (water–gas reaction), the pressure-form expression is

21 / 30

21. In at constant temperature, the equilibrium constant is numerically equal to

22 / 30

22. According to Arrhenius, which of the following aqueous solutions has the highest concentration of ions?

23 / 30

23. For a gaseous system, the reaction quotient in terms of partial pressure is represented as

24 / 30

24. For a reaction at temperature (T), which equation connects the definition of equilibrium with thermodynamics?

25 / 30

25. For the reaction , what type of equilibrium is established?

26 / 30

26. The relationship between hydrolysis constant , degree of hydrolysis (h), and concentration (C) for a salt of a weak acid and strong base is

27 / 30

27. When a reversible reaction attains equilibrium, what remains constant?

28 / 30

28. For at 298 K, . The predicted extent toward (B) is

29 / 30

29. The Arrhenius concept is limited to

30 / 30

30. A nonvolatile solute is dissolved in a solvent with at a given (T). If the solute mole fraction is , the solution’s vapour pressure is:

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Class 11 Chemistry: Equilibrium Online Test (Paper 3)

Welcome to Paper 3! You’ve warmed up—now it's time to step up your game and conquer the challenge with tougher questions!

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  • Total Questions: 50
  • Time Allotted: 75 minutes
  • Passing Score: 70%
  • Randomization: Yes
  • Certificate: Yes
  • Retake: Allowed
  • Price: 100% Free

Good luck! 👍

1 / 50

1. The equilibrium is homogeneous because

2 / 50

2. For , if initial concentrations of all species are and , the equilibrium will be

3 / 50

3. In rigorous thermodynamic form, the law of mass action is written with:

4 / 50

4. If for a base, the strength of the base is

5 / 50

5. In the Haber process , increasing the pressure will

6 / 50

6. The molar solubility (S) of a salt in terms of is

7 / 50

7. Which of the following is not a weak electrolyte?

8 / 50

8. For , the mass-action expressions are and . At equilibrium, the condition implied is:

9 / 50

9. The pair is an example of

10 / 50

10. The (pH) of a salt solution formed by a weak acid and strong base can be expressed as

11 / 50

11. In the reaction , if and , the reaction will

12 / 50

12. The equilibrium constant for the homogeneous reaction is expressed as

13 / 50

13. In , adding solid to an already saturated solution at fixed (T) will

14 / 50

14. For an exothermic reaction, increasing temperature will shift equilibrium

15 / 50

15. For a weak acid with small , the degree of ionization is approximately proportional to

16 / 50

16. Strong bases are those that

17 / 50

17. For an endothermic reaction, decreasing temperature causes

18 / 50

18. For , with and initial , equilibrium is

19 / 50

19. Which of the following pairs does not form a buffer solution?

20 / 50

20. The reversible decomposition of calcium carbonate is an example of:

21 / 50

21. For the reaction with and initial , the equilibrium concentration of (HI) is

22 / 50

22. For a system at constant (T) and (P), a spontaneous process always has

23 / 50

23. The expression for the hydrolysis constant of a salt of a weak base and a strong acid is

24 / 50

24. The (pH) of a (0.01,M) (NaOH) solution is

25 / 50

25. According to Arrhenius, which of the following aqueous solutions has the highest concentration of ions?

26 / 50

26. In the Contact process, lowering the temperature increases the yield of because the reaction is

27 / 50

27. The importance of Henderson’s equation lies in the fact that it

28 / 50

28. For a salt of a weak acid and a weak base , the hydrolysis constant is

29 / 50

29. The salt formed from (NaOH) and (HCl) will have a pH value of

30 / 50

30. The degree of hydrolysis ((h)) of a salt of a weak acid and strong base is given by

31 / 50

31. When a reversible reaction attains equilibrium, what remains constant?

32 / 50

32. When equilibrium is reached in the reaction , what best explains macroscopic constancy?

33 / 50

33. Which of the following acids is weak?

34 / 50

34. The common ion effect is an application of

35 / 50

35. For , if initial and , the equilibrium is

36 / 50

36. For a weak acid where is very small, Ostwald’s dilution law simplifies to

37 / 50

37. The of (AgCl) is expressed as

38 / 50

38. In the Haber process, lowering the temperature will

39 / 50

39. If , the reaction will proceed

40 / 50

40. The Haber process is exothermic. Which change increases the equilibrium yield of ?

41 / 50

41. In a closed container at fixed (T), liquid–vapour equilibrium is reached when:

42 / 50

42. Which statement about a catalyst and equilibrium is correct?

43 / 50

43. The product of and ( C ) for a weak acid at a given temperature is

44 / 50

44. The relationship between and for a gas-phase equilibrium is:

45 / 50

45. For the reaction , the equilibrium constant in terms of concentration is derived by equating:

46 / 50

46. Which of the following is a weak electrolyte?

47 / 50

47. For an ideal binary solution of volatile components (A) and (B), Raoult’s law states:

48 / 50

48. In a gaseous equilibrium, decreasing the concentration of reactants will cause

49 / 50

49. The ionization constant of acetic acid is . This indicates it is

50 / 50

50. For the dissociation , the correct mass-action expression in pressure terms is:

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Practice Equilibrium MCQs
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Class 11 Chemistry — Chapter 7: Equilibrium Online Test

The Class 11 Chemistry: Chapter 7 – Equilibrium Online Test offers a comprehensive pool of 400 MCQs designed to strengthen your understanding of chemical equilibrium. This test is free, aligned with the CBSE/NCERT syllabus, and allows you to take unlimited attempts to assess and improve your grasp of equilibrium concepts.

Nervous about mastering equilibrium concepts? This online test is the perfect solution to practice at your own pace. Whether you’re looking to revise the Law of Mass Action, Le-Chatelier’s Principle, or understand ionic equilibrium, this test will guide you step by step. Each attempt gives you a real-time score and the opportunity to review and learn from your mistakes. Plus, passing Paper 3 will earn you a certificate to mark your progress!

What is this Class 11 Chemistry: Equilibrium Online Test?

This page contains three exam-style MCQ papers for Chapter 7: Equilibrium:

  • Paper 1 (Easy) — Foundation: 20 questions · 30 min · Pass 40% · Fixed set
  • Paper 2 (Medium) — Mixed: 30 questions · 45 min · Pass 50% · Randomized from a pool of 400 questions
  • Paper 3 (Hard) — Challenge: 50 questions · 75 min · Pass 70% · Randomized from the same pool + Certificate on pass

Note: Paper 2 and Paper 3 offer a fresh set of questions each time you take the test, with randomized questions ensuring varied practice each attempt. All papers are timed and auto-evaluated, giving you instant feedback.

Topics Covered in these Online Tests

The online test for Chapter 7: Equilibrium covers various critical sub-topics that will be assessed in your exams. Here’s what you can expect:

  • Dynamic Nature of Equilibrium — Understanding the reversibility of reactions and the concept of equilibrium state
  • Law of Chemical Equilibrium — Mathematical expression, Kc, Kp, and their applications
  • Le-Chatelier’s Principle — How changes in concentration, temperature, and pressure affect equilibrium
  • Equilibrium Constant (K) — Relationship between Kc and Kp, and how to calculate equilibrium constants
  • Ionic Equilibrium — Dissociation of acids and bases, strong and weak electrolytes
  • Buffer Solutions — Definition, buffer capacity, and examples
  • pH and pOH — Calculations and their role in equilibria
  • Common Ion Effect — Impact of adding a common ion to a solution at equilibrium
  • Solubility Product — Applications and calculations of Ksp, common examples like sparingly soluble salts
  • Complex Equilibria — Formation constants and equilibrium involving complex ions

This is just a preview of the core topics covered. You can also find more detailed study material and MCQs for Chapter 7 in the full MCQ Question Bank.

How This Exam-Style Online Test Works

  • Pick a paper → Answer MCQs within the time limit → Submit → Get instant score and answer review.
  • Timed MCQs: Paper 1 is 30 minutes, Paper 2 is 45 minutes, and Paper 3 is 75 minutes.
  • Instant Feedback: See your score immediately, with an option to review your answers and explanations for better understanding.
  • Unlimited Retakes: You can retake the test as many times as you like, with new randomized questions in Paper 2 and Paper 3.
  • Certificate on passing Paper 3: After scoring 70% or more in Paper 3, you can earn a certificate.

What you’ll see during the test

  • MCQs: One question with four options (A, B, C, D).
  • Timer: P1: 30 min · P2: 45 min · P3: 75 min.
  • Pagination: Typically 10 questions per page (navigate to the next set using page controls).
  • Navigation: Use Next/Prev buttons or the question map to go back before submitting.
  • View Result: Click View Result to see your score and a detailed summary.
  • Result page: Shows your score %, correct/incorrect/unanswered count, answer key, and a share button.
  • Restart: Click Restart Test to try again with a new mix of questions (Paper 2 & Paper 3).

Note: Please share your feedback on the result page after completing a test.

Marking & Pass Criteria

  • Scoring: +1 for correct answers, 0 for incorrect (no negative marking).
  • Passing marks: Paper 1 — 40% • Paper 2 — 50% • Paper 3 — 70%.
  • Randomization: Paper 2 & Paper 3 shuffle questions from the large pool of 400 MCQs on every attempt. Paper 1 stays fixed.

Who can take this test?

  • Class 11 CBSE/NCERT students studying Chapter 7: Equilibrium.
  • JEE/NEET aspirants strengthening their grasp of equilibrium for competitive exams.
  • Teachers and tutors looking for chapter-specific MCQ tests for class assessments.
  • International students studying under IGCSE, IB, AP, O/A-Levels systems, wanting to reinforce core Chemistry concepts.
  • Self-learners or home-schoolers seeking structured, easy-to-use online tests to practice key Chemistry concepts.

Advantages of this Online Test

  • Exam-like feel: Timed tests, pass percentage, and auto-submit features simulate real exam conditions.
  • Instant feedback: Gain immediate insights into your performance with a detailed result summary.
  • Step-up difficulty: Start with Paper 1 (easy), move to Paper 2 (medium), and challenge yourself with Paper 3 (hard). Get a certificate after passing Paper 3.
  • Unlimited attempts: Practice as many times as you need with fresh randomized questions in Paper 2 and Paper 3.
  • Zero cost: Completely free; no hidden charges or sign-ins required.

How this test helps you study better

  • Step 1 – Concept check: Attempt Paper 1 to test your basic understanding of equilibrium principles.
  • Step 2 – Reinforce: Move to Paper 2 for a more mixed set of questions to stabilize your accuracy.
  • Step 3 – Full exam readiness: Attempt Paper 3 to simulate a real exam environment and aim for ≥ 70% to earn your certificate.
  • Step 4 – Review: Analyze your mistakes and revise only the concepts you missed.
  • Step 5 – Retake smartly: Re-attempt after a break to gauge long-term retention of the material.

Important Notes (Read Before You Start)

  • Do not refresh or close the tab during the test.
  • Best experience: Use Chrome/Edge with a stable internet connection.
  • Allow cookies/local storage for smooth progress saving and session continuity.
  • Safety: This test is 100% FREE and safe—ignore any payment requests.

More Practice for Class 11 Chemistry

After completing this test, you can strengthen your understanding further by visiting: Class 11 Chemistry MCQs or view the entire Class 11 Chemistry Online Test Index.

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