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

2 / 30

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

3 / 30

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

4 / 30

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

5 / 30

5. A gas occupies 4 L at 2 atm. What will be its volume at 1 atm and constant temperature?

6 / 30

6. Which of the following order of strength is correct for intermolecular forces?

7 / 30

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

8 / 30

8. Which statement best describes the internal arrangement (“order”) of particles?

9 / 30

9. Which phenomenon in plants is partially explained by surface tension?

10 / 30

10. Which condition favors ideal behavior most strongly?

11 / 30

11. At the same temperature, which gas has the highest RMS speed?

12 / 30

12. Why do metals typically have high melting and boiling points?

13 / 30

13. Which liquid has the highest surface tension at room temperature?

14 / 30

14. In the above question, what is the partial pressure of oxygen?

15 / 30

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

16 / 30

16. Two flasks of equal volume contain equal masses of hydrogen and oxygen at the same T and P. Which statement is correct?

17 / 30

17. Why do small insects like water striders walk on water without sinking?

18 / 30

18. At temperatures above the critical temperature, Andrews found that:

19 / 30

19. The average translational kinetic energy per mole of a gas is given by:

20 / 30

20. A flask at contains mol and mol . What is the total pressure?

21 / 30

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

22 / 30

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

23 / 30

23. London dispersion forces arise due to:

24 / 30

24. A 2 L container has 0.50 mol of and 0.50 mol of at 300 K. The total pressure is 24.6 atm. What is the partial pressure of each gas?

25 / 30

25. Dalton’s law can be combined with the ideal gas equation to give:

26 / 30

26. Which law explains why an inflated football shrinks when taken from a warm room into a cold environment?

27 / 30

27. A sample of H₂ effuses through a hole in 10 minutes. Under same conditions, how long will it take the same volume of methane (CH₄, M=16) to effuse?

28 / 30

28. Which type of gas will have a higher value of ?

29 / 30

29. What is the density of at and ? ()

30 / 30

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

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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!

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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. Why do solids have fixed shape compared to liquids and gases?

2 / 50

2. Effusion of a gas refers to:

3 / 50

3. If the volume of a gas is 600 mL at 300 K, what will be the volume at 600 K at constant pressure?

4 / 50

4. Which has stronger intermolecular forces: or ?

5 / 50

5. Which of the following order of strength is correct for intermolecular forces?

6 / 50

6. A 2 L flask contains O₂ at 3 atm and a 3 L flask contains H₂ at 4 atm, both at same temperature. If gases are mixed in a 5 L vessel, what is the total pressure?

7 / 50

7. What volume will mol occupy at and ?

8 / 50

8. For a non-polar gas like helium, deviation from ideality is mainly due to:

9 / 50

9. The mathematical form of Avogadro’s law is:

10 / 50

10. Why does the pressure inside a sealed aerosol can increase when exposed to sunlight?

11 / 50

11. The coefficient of viscosity is related to viscous drag force by the equation:

12 / 50

12. The coefficient of volume expansion is generally in the order:

13 / 50

13. What is the compressibility factor for an ideal gas?

14 / 50

14. Why are liquid crystals important in modern technology?

15 / 50

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

16 / 50

16. In the smectic phase of liquid crystals, molecules are:

17 / 50

17. A gas has pressure of 2 atm at 300 K. What will be its pressure at 450 K if volume is constant?

18 / 50

18. Which phenomenon in plants is partially explained by surface tension?

19 / 50

19. For an ideal gas, how does the vs plot appear at constant temperature?

20 / 50

20. A mixture of gases at 27°C and 1 atm contains 0.4 mol of and 0.6 mol of . What is the partial pressure of nitrogen?

21 / 50

21. In compressibility factor vs curves, for an ideal gas:

22 / 50

22. Which postulate of the kinetic molecular theory explains the pressure exerted by gases?

23 / 50

23. Two flasks of equal volume contain equal masses of hydrogen and oxygen at the same T and P. Which statement is correct?

24 / 50

24. Which concept explains why liquefaction of gases is possible at low temperature and high pressure?

25 / 50

25. The average translational kinetic energy per mole of a gas is given by:

26 / 50

26. Which condition favors ideal behavior most strongly?

27 / 50

27. Which of the following optical property is unique to liquid crystals?

28 / 50

28. A mixture of CH₄ and He diffuses through a hole. If the mixture diffuses 1.5 times faster than O₂, calculate the mole fraction of CH₄. (MCH₄ = 16, MHe = 4, MO₂ = 32).

29 / 50

29. Which relation connects pressure and average kinetic energy of molecules?

30 / 50

30. Why does heating a sealed glass container sometimes cause it to shatter?

31 / 50

31. Why do small liquid drops form spherical shapes?

32 / 50

32. 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?

33 / 50

33. The intercept of the extrapolated Volume vs Temperature (°C) graph of a gas is:

34 / 50

34. Which step is essential in deriving the kinetic theory equation for pressure?

35 / 50

35. Which statement about boiling and evaporation is correct?

36 / 50

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

37 / 50

37. Which gas has the highest critical temperature among the following?

38 / 50

38. Which of the following mixtures obeys Avogadro’s law most accurately?

39 / 50

39. Which assumption of kinetic theory best explains why gases have very low densities compared to liquids and solids?

40 / 50

40. Which assumption of kinetic theory explains why gases have neither definite shape nor definite volume?

41 / 50

41. The heat absorbed during the conversion of 1 mole of ice at to water at is called:

42 / 50

42. Surface tension of a liquid is defined as:

43 / 50

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

44 / 50

44. Which property of gases is explained by Graham’s law?

45 / 50

45. For a real gas, indicates:

46 / 50

46. Which force is dominant in the interaction between ion and molecule?

47 / 50

47. Which factor is more significant at low pressure?

48 / 50

48. The average speed of gas molecules is given by:

49 / 50

49. Gay Lussac’s law states that for a fixed mass of gas at constant volume:

50 / 50

50. The mathematical expression for Charles’ law is:

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Practice States of Matter MCQs
Download Class 11 Chemistry MCQ Study Bundle

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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