Exam-Style Online Test | Class 11 Chemistry: Equilibrium
GKaim: Measure. Improve. Achieve.

Class 11 Chemistry — Chapter 7: Equilibrium Online Test

Start Your Test by Choosing a Paper

0%

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

Good luck! 👍

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:

Please provide information to view your result.

Your score is

Share your achievement!

LinkedIn Facebook
0%

Please provide your feedback.

Thank you for your valuable feedback.

0%

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.

Get new questions on each attempt

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

Good luck! 👍

1 / 30

1. The reaction is a homogeneous equilibrium because

2 / 30

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

3 / 30

3. When , the relation between and becomes

4 / 30

4. For the decomposition at equilibrium, which is true?

5 / 30

5. For the decomposition reaction , the equilibrium constant is derived as:

6 / 30

6. The conjugate base of is

7 / 30

7. The Henderson–Hasselbalch equation is derived from

8 / 30

8. The Contact process involves the oxidation of to : . Increasing pressure will

9 / 30

9. If , the hydroxide ion concentration is

10 / 30

10. Which statement differentiates “dynamic” chemical equilibrium from “static” equilibrium?

11 / 30

11. Which is a correct necessary condition embedded in the definition of chemical equilibrium for a gas-phase reaction?

12 / 30

12. For , lowering temperature generally leads to

13 / 30

13. The pH of ammonium acetate depends on

14 / 30

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

15 / 30

15. The pH of sodium acetate solution is

16 / 30

16. Which of the following pairs correctly shows the order of increasing ionization?

17 / 30

17. For gases behaving ideally, the mass-action expression in terms of partial pressures for is:

18 / 30

18. Why does a chemical system at equilibrium appear static to the observer?

19 / 30

19. When the concentration of products is increased at equilibrium, the system

20 / 30

20. Consider with at 298 K. Starting from , the expected equilibrium is

21 / 30

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

22 / 30

22. In the Haber process, lowering the temperature will

23 / 30

23. When a solution is just saturated with a salt, the ionic product is

24 / 30

24. The unit of for the reaction is

25 / 30

25. Which of the following statements correctly describes acetic acid solution?

26 / 30

26. The law of mass action at equilibrium for states that the ratio is:

27 / 30

27. The strength of an acid is determined by the magnitude of its

28 / 30

28. In qualitative analysis, group II cations like , , and are precipitated as sulfides in acidic medium because

29 / 30

29. For the reaction , the relation between and is

30 / 30

30. The salt of a weak acid and weak base gives a solution that is

Please provide information to view your result.

Your score is

Share your achievement!

LinkedIn Facebook
0%

Please provide your feedback.

Thank you for your valuable feedback.

0%

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!

Earn a certificate upon passing

Get new questions with every attempt

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

Good luck! 👍

1 / 50

1. If , the reaction will proceed

2 / 50

2. If , the reaction will

3 / 50

3. The larger the value of , the

4 / 50

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

5 / 50

5. The equilibrium condition can be derived from the expression

6 / 50

6. A solution with has hydrogen ion concentration

7 / 50

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

8 / 50

8. The main difference between a weak acid and a weak electrolyte is that

9 / 50

9. For an endothermic reaction, increasing temperature shifts equilibrium

10 / 50

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

11 / 50

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

12 / 50

12. The degree of ionization of an electrolyte is higher in solvents having

13 / 50

13. For an endothermic reaction, decreasing temperature causes

14 / 50

14. Which of the following statements about and is true?

15 / 50

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

16 / 50

16. Which condition is required for a reversible reaction to reach equilibrium?

17 / 50

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

18 / 50

18. Which condition is inherently included in the definition of equilibrium for a reaction mixture?

19 / 50

19. A sealed flask contains at temperature (T). Doubling the mass of while keeping (T) fixed will

20 / 50

20. The Contact process involves the oxidation of to : . Increasing pressure will

21 / 50

21. If the dielectric constant of a medium increases, the force of attraction between ions

22 / 50

22. According to Le Chatelier’s principle, if the concentration of a reactant is increased, the system will

23 / 50

23. If , the hydroxide ion concentration is

24 / 50

24. Which of the following is a strong acid?

25 / 50

25. When the ionic product (Q) of a salt solution exceeds , it means

26 / 50

26. If for a gaseous reaction, the relation between and is:

27 / 50

27. For at 298 K with and initial , the direction to reach equilibrium is

28 / 50

28. If the of is , then the of its conjugate acid is

29 / 50

29. For a salt , the relationship between and molar solubility (S) is

30 / 50

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

31 / 50

31. Consider in a closed vessel. The equilibrium constant depends on

32 / 50

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

33 / 50

33. In a buffer containing and , the pH is calculated using

34 / 50

34. In the reaction , the equilibrium is

35 / 50

35. Which of the following has the smallest degree of ionization in water?

36 / 50

36. The relation between and obtained from the mass-action law for a gas reaction is:

37 / 50

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

38 / 50

38. According to the Brønsted–Lowry concept, a base is a substance that

39 / 50

39. In the equilibrium , the equilibrium constant in pressure form is

40 / 50

40. The conjugate base of a strong acid is always

41 / 50

41. For , the correct expression for is

42 / 50

42. A reaction is spontaneous in the forward direction when

43 / 50

43. Which of the following graphs best represents Ostwald’s dilution law?

44 / 50

44. The relation between hydrogen ion concentration and the initial concentration ( C ) of a weak acid is

45 / 50

45. Temperature affects the mass-action constant because:

46 / 50

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

47 / 50

47. According to Lewis acidity/basicity trends, which order of acid strength is most reasonable toward a hard donor like ?

48 / 50

48. According to the Brønsted–Lowry concept, an acid is a substance that

49 / 50

49. When , the relation between and becomes

50 / 50

50. A closed flask containing water at shows constant vapour pressure. Which measurement provides direct evidence that liquid–vapour equilibrium is dynamic?

Please provide accurate information so we can send your Achievement Certificate by mail.

Your score is

Share your achievement!

LinkedIn Facebook
0%

Please provide your feedback.

Thank you for your valuable feedback.

Practice Equilibrium MCQs
Download Class 11 Chemistry MCQ Study Bundle

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.

FAQs on Equilibrium Online Test ▼

Subscribe
Notify of
guest
0 Comments

Related MCQs

Scroll to Top