Exam-Style Online Test | Class 11: States Of Matter Test

Class 11 Chemistry — Chapter 5: States of Matter Online Test

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Class 11 Chemistry: States of Matter 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. A rigid vessel at contains mol and mol . An electric spark causes complete reaction . After cooling back to , what is the final pressure?

2 / 20

2. Which property makes supercritical fluids useful as solvents in industry?

3 / 20

3. Which curve best represents the relation between vapour pressure and temperature?

4 / 20

4. What is the critical temperature of CO₂ observed in Andrews’ experiments?

5 / 20

5. The van der Waals constant has which units (for 1 mol gas)?

6 / 20

6. Why is added to pressure in the van der Waals equation?

7 / 20

7. At very low pressure, the compressibility factor of a real gas approaches:

8 / 20

8. If for a gas, it means:

9 / 20

9. If hydrogen () has an RMS speed of 1840 m/s at a given temperature, what is the RMS speed of oxygen () at the same temperature?

10 / 20

10. Which relation connects pressure, volume, and average kinetic energy of molecules?

11 / 20

11. Which constant directly connects molecular kinetic energy with absolute temperature?

12 / 20

12. Which assumption of kinetic theory explains the compressibility of gases?

13 / 20

13. Which of the following statements is correct about Dalton’s law?

14 / 20

14. If 3 L of nitrogen gas contains molecules at constant T and P, how many molecules will 6 L of nitrogen contain?

15 / 20

15. Which statement is true about Avogadro’s number ()?

16 / 20

16. The graph of Gay Lussac’s law (Pressure vs Temperature) is:

17 / 20

17. Which everyday example best demonstrates Charles’ law?

18 / 20

18. Boyle’s law is valid under which condition?

19 / 20

19. Which has stronger intermolecular forces: or ?

20 / 20

20. The correct order of diffusion rate at room temperature is:

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Class 11 Chemistry: States of Matter 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. Why does graphite have a very high melting point?

2 / 30

2. Which real-life example demonstrates Avogadro’s law?

3 / 30

3. In the van der Waals equation, the constant represents:

4 / 30

4. Supercritical CO₂ is used in green chemistry because:

5 / 30

5. Which property of gases can be predicted using critical constants?

6 / 30

6. Andrews’ experiments on CO₂ demonstrated the concept of:

7 / 30

7. What makes liquid crystals fundamentally important in modern materials science?

8 / 30

8. Why does a football appear deflated when taken out on a cold winter morning?

9 / 30

9. Which example demonstrates thermal energy being reduced until intermolecular forces dominate?

10 / 30

10. Which important conclusion arises from the derivation of the pressure equation?

11 / 30

11. What happens to the viscosity of liquids when strong intermolecular hydrogen bonding is present?

12 / 30

12. A scuba tank contains 80% N₂ and 20% O₂ at 10 atm. What is the partial pressure of O₂?

13 / 30

13. Cholesteric (chiral nematic) liquid crystals are characterized by:

14 / 30

14. The temperature at which vapour pressure of a liquid equals atmospheric pressure is called:

15 / 30

15. What volume will mol occupy at and ?

16 / 30

16. A binary mixture of and effuses times faster than pure at the same and . What is the mole fraction of in the mixture?

17 / 30

17. Which of the following correctly arranges intermolecular forces in increasing order of strength?

18 / 30

18. Which formula relates partial pressure of a gas to its mole fraction?

19 / 30

19. According to Poiseuille’s equation, viscosity of a liquid is directly proportional to:

20 / 30

20. Why does water have a much higher boiling point than hydrogen sulfide ()?

21 / 30

21. A gas sample has volume 2.0 L at 300 K. What will be its volume at 450 K if pressure remains constant?

22 / 30

22. In scuba diving, the composition of compressed air cylinders must consider Dalton’s law because:

23 / 30

23. Why is knowledge of important in industry?

24 / 30

24. Which state of matter has definite volume but no definite shape?

25 / 30

25. Which of the following best explains why compressibility factor is useful?

26 / 30

26. Which property makes supercritical fluids useful as solvents in industry?

27 / 30

27. The critical temperature () of a gas is defined as:

28 / 30

28. Why do gases deviate from ideality at high pressure?

29 / 30

29. Effusion of a gas refers to:

30 / 30

30. Which intermolecular force determines the liquefaction ease of ?

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Class 11 Chemistry: States of Matter 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

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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 capillary rise of water is due to:

2 / 50

2. The average kinetic energy of molecules in 1 mol of gas at 27°C is approximately:

3 / 50

3. The critical constants () are related to which equation of state?

4 / 50

4. The temperature at which a gas theoretically occupies zero volume is called:

5 / 50

5. A mixture contains 1 mol of O₂ and 2 mol of He at total pressure 12 atm. What is partial pressure of O₂?

6 / 50

6. Which relation is correct for diffusion rates of gases A and B?

7 / 50

7. Which of the following relations between molecular speeds is correct for an ideal gas?

8 / 50

8. The work required to increase the surface area of a liquid by 1 unit is equal to:

9 / 50

9. Why is the boiling point of HF higher than HCl, though HCl has greater molar mass?

10 / 50

10. Which gas shows the largest negative deviation () under ordinary conditions?

11 / 50

11. Which compound has the highest boiling point due to intermolecular forces?

12 / 50

12. Which important conclusion arises from the derivation of the pressure equation?

13 / 50

13. The constant obtained in Boyle’s law, , depends on:

14 / 50

14. In collecting gas over water, the measured pressure includes:

15 / 50

15. Why does the pressure inside a car tire increase when the car is driven for a long distance?

16 / 50

16. The minimum point in a vs curve (below unity) corresponds to:

17 / 50

17. If 2 L of gas reacts completely with 1 L of gas at the same T and P, the volume of vapor formed will be:

18 / 50

18. Why does viscosity of gases increase with temperature, unlike liquids?

19 / 50

19. A balloon filled with 2 mol of H₂ and 2 mol of O₂ is at 300 K and 5 atm total pressure. What is the partial pressure of H₂?

20 / 50

20. Which situation illustrates intermolecular forces dominating over thermal energy?

21 / 50

21. At constant T and P, 1 L of H₂ contains 0.04 mol. How many liters of O₂ at same T and P will contain 0.08 mol?

22 / 50

22. Which expression correctly represents Avogadro’s law?

23 / 50

23. In Andrews’ experiment, what happened to CO₂ when pressure was increased at a temperature below its critical temperature?

24 / 50

24. Which real-life application uses Graham’s law of diffusion?

25 / 50

25. A gas sample initially at 1 atm and 500 mL is compressed isothermally to 250 mL. The final pressure is:

26 / 50

26. Viscosity of a liquid is defined as:

27 / 50

27. Which constant directly connects molecular kinetic energy with absolute temperature?

28 / 50

28. At very low pressures, the compressibility factor of real gases approaches unity because:

29 / 50

29. What is the effect of adding impurities like electrolytes on viscosity of water?

30 / 50

30. What phenomenon did Andrews’ experiments directly demonstrate for the first time?

31 / 50

31. A fixed mass of gas expands from to at the same temperature. The ratio of final to initial density is:

32 / 50

32. Which of the following experimental setups best verifies Boyle’s law?

33 / 50

33. Which property of supercritical fluids is closer to liquids?

34 / 50

34. Why do molecular solids like naphthalene have relatively low melting points compared to ionic solids?

35 / 50

35. A gas has density at STP. Its molar mass is approximately:

36 / 50

36. Which interaction is responsible for the solubility of ionic compounds in polar solvents?

37 / 50

37. 1 L of H₂ effuses through a hole in 10 minutes. How long will it take for the same volume of CO₂ (M = 44) under identical conditions?

38 / 50

38. Which equation relates surface tension () to rise of liquid in a capillary?

39 / 50

39. Which factor does not significantly influence the viscosity of a liquid?

40 / 50

40. The value of for CO₂ at moderate pressures is often less than 1. This indicates:

41 / 50

41. Supercritical CO₂ is used in green chemistry because:

42 / 50

42. Which everyday example best demonstrates Charles’ law?

43 / 50

43. Which of the following best explains Brownian motion?

44 / 50

44. A gas mixture of 5 mol and 3 mol exerts a total pressure of 4 atm. What is the partial pressure of oxygen?

45 / 50

45. Relative viscosity of two liquids (1 and 2) using Ostwald viscometer is given by:

46 / 50

46. Which factor mainly affects the rate of evaporation of a liquid?

47 / 50

47. At what temperature will the average kinetic energy of oxygen molecules be twice that at 300 K?

48 / 50

48. Which of the following liquids forms a convex meniscus in a glass capillary?

49 / 50

49. The graph of Gay Lussac’s law (Pressure vs Temperature) is:

50 / 50

50. Why does boiling point increase as we move from helium to xenon among noble gases?

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Practice States of Matter MCQs
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Class 11 Chemistry — Chapter 5: States of Matter Online Test

Welcome to the Class 11 Chemistry: Chapter 5 – States of Matter Online Test page. This test offers a collection of 494 MCQs that cover the essential concepts of the states of matter, including gases, liquids, and solids. The online test is designed to help you strengthen your understanding and master the key topics in this chapter. It is free, aligned with the CBSE/NCERT curriculum, and available for unlimited attempts. Each paper is timed, and you will get instant feedback after each attempt.

Struggling with the gas laws, or trying to understand intermolecular forces? This test is an excellent way to practice and prepare yourself for upcoming exams. Think of this as your personal online mock test for the States of Matter chapter, available anytime on your phone or computer. Whether you’re a beginner or an advanced learner, you can progress through the Easy, Medium, and Hard levels, and track your improvements as you go.

What is this Class 11 Chemistry: States of Matter Online Test?

This page features three different difficulty levels of the MCQ test for Chapter 5:

  • 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 ~494 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 are randomized, so you’ll get a new set of questions on each attempt. The test is timed, and once you submit your answers, you’ll instantly see your score and a review of your responses.

Topics covered in these online tests

This test focuses on essential topics in Chapter 5, which covers the three states of matter and their properties. The main concepts that you will practice include:

  • Properties of Gases — Ideal gas law, gas laws, Boyle’s law, Charles’ law, and real gases
  • Ideal Gas Equation — PV = nRT, applications of the ideal gas equation
  • Liquids — Properties of liquids, viscosity, surface tension, and capillarity
  • Solids — Properties of solids, crystal lattices, and unit cells
  • Intermolecular Forces — Types of forces, dipole-dipole interactions, hydrogen bonding, London dispersion forces
  • Gas Laws & Kinetic Molecular Theory — Kinetic theory of gases, deviations from ideal gas behavior, Maxwell’s distribution of velocities
  • Liquefaction of Gases — Critical temperature, critical pressure, Van der Waals equation of state
  • Real Gases — Compressibility factor, deviations from ideal gas behavior
  • Surface Chemistry — Adsorption, adsorption isotherms, catalysis

How This Exam-Style Online Test Works

Simple Steps: Select a paper → Answer the questions within the time limit → Submit → View your results instantly with a detailed breakdown.

What you’ll experience in this test

  • MCQs: One question with four possible answers (A, B, C, D).
  • Timer on top: Paper 1: 30 minutes • Paper 2: 45 minutes • Paper 3: 75 minutes.
  • Pagination: Typically 10 questions per page. Use navigation to move between questions.
  • Answer Review: After finishing the test, you’ll receive your score, along with the correct answers and detailed explanations.
  • Instant Feedback: Click View Result to see your score, and review the questions you answered incorrectly.
  • Retake Option: Click Restart Test to try again with a new set of questions (Paper 2 & 3).

Note: Share your feedback on the result page after completing the test to help us improve.

Marking & Pass Criteria

  • Scoring: +1 for every correct answer, 0 for incorrect (no negative marking).
  • Passing Marks: Paper 1 — 40% • Paper 2 — 50% • Paper 3 — 70%.
  • Randomization: Paper 2 & Paper 3 will shuffle questions from a pool of ~494 questions. Paper 1 remains fixed.

Who can take this test?

  • Class 11 CBSE students preparing for unit tests, half-yearlies, and final exams.
  • Class 12 bridge students revising basic concepts of States of Matter.
  • JEE/NEET aspirants focusing on understanding gas laws, properties of gases, and real gases for competitive exams.
  • School teachers / tutors needing a ready-to-use, chapter-specific test for homework, practice, or revision.
  • Self-learners and homeschoolers who wish to test their knowledge and improve concepts.

Benefits of this online test

  • Exam-like experience: Get a feel for timed, exam-style questions with real-time feedback.
  • Instant results: Learn from your mistakes immediately after each attempt.
  • Stepped-up difficulty: Start with the basics, progress to intermediate questions, and challenge yourself with harder ones.
  • Unlimited attempts: Practice as often as you like to improve speed and accuracy.
  • Zero cost: No fees or hidden charges — completely free for all students.

How this test can help you study better

  • Step 1 – Initial understanding: Try Paper 1 to check your knowledge on fundamental concepts.
  • Step 2 – Consolidate learning: Move to Paper 2 (randomized) to cover intermediate-level questions.
  • Step 3 – Challenge yourself: Attempt Paper 3 to strengthen exam-readiness with tougher questions.
  • Step 4 – Review mistakes: Revisit wrong answers, learn from them, and improve your accuracy.

Important Notes (read before starting)

  • Do not refresh or close the test tab to avoid losing progress.
  • Best experience: Use a modern browser (Chrome/Edge), stable internet connection, and a distraction-free environment.
  • Allow cookies / local storage for smooth tracking of progress and results.
  • Safety: This test is 100% FREE, and there are no hidden charges.

Additional Practice for Class 11 Chemistry

To continue your preparation, explore the full collection of Class 11 Chemistry MCQs: Class 11 Chemistry Online Test Index or practice all chapters from the Class 11 Chemistry MCQ Collection.

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