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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. For 1 mole of a gas, the van der Waals equation is:

2 / 30

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

3 / 30

3. Liquids with stronger intermolecular forces will have:

4 / 30

4. The critical volume () refers to:

5 / 30

5. Hydrogen diffuses four times faster than which of the following gases?

6 / 30

6. Why does high pressure promote liquefaction of gases?

7 / 30

7. Boyle’s law can be stated as:

8 / 30

8. Which of the following statements about liquid crystal displays (LCDs) is correct?

9 / 30

9. Why must temperature always be measured in Kelvin when applying Gay Lussac’s law?

10 / 30

10. Which real-life application depends on Boyle’s law?

11 / 30

11. How does viscosity of gases change with temperature?

12 / 30

12. Which interaction explains the high solubility of salts in water?

13 / 30

13. What happens to the volume of a gas if temperature is reduced to half at constant pressure?

14 / 30

14. Which gas behaves most ideally under ordinary conditions?

15 / 30

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

16 / 30

16. Surface tension is measured in SI units as:

17 / 30

17. Effusion of a gas refers to:

18 / 30

18. Which condition makes the van der Waals equation reduce to the ideal gas law?

19 / 30

19. In an experiment, two gases diffuse through the same pinhole. If gas A takes 36 s and gas B takes 64 s, the ratio of their molar masses () is:

20 / 30

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

21 / 30

21. A supercritical fluid is defined as:

22 / 30

22. The Boyle temperature of a gas is defined as:

23 / 30

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

24 / 30

24. Which statement about densities is correct?

25 / 30

25. A gas has a volume of 4.0 L at 27°C. What will be its volume at 127°C, keeping pressure constant?

26 / 30

26. Why are liquid crystals important in modern technology?

27 / 30

27. Unit of viscosity in the CGS system is:

28 / 30

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

29 / 30

29. Why does Dalton’s law fail for real gases at high pressure?

30 / 30

30. The expression for the most probable speed () is:

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

Good luck! 👍

1 / 50

1. For nitrogen gas at 300 K, the three molecular speeds are approximately:

2 / 50

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

3 / 50

3. If 1 mole of gas occupies 22.4 L at STP, how many liters will 2 moles occupy at the same conditions?

4 / 50

4. The direct conversion of water vapor into ice without becoming liquid is known as:

5 / 50

5. Which of the following is measured by a thermometer?

6 / 50

6. Why do liquids evaporate even at temperatures below their boiling point?

7 / 50

7. Viscosity of a liquid is defined as:

8 / 50

8. Which of the following is an example of thermal energy dominating over intermolecular forces?

9 / 50

9. Why is the critical temperature () important in the liquefaction of gases?

10 / 50

10. A balloon filled with air at 1 atm has a volume of 2.5 L. If the balloon is squeezed until volume becomes 1.25 L, the new pressure inside will be:

11 / 50

11. Vapour pressure of a liquid increases with:

12 / 50

12. Why does ammonia gas deviate strongly from ideal behavior?

13 / 50

13. The bends (decompression sickness) in divers is caused mainly due to:

14 / 50

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

15 / 50

15. The functioning of LCD screens is based on:

16 / 50

16. Which has stronger intermolecular forces: or ?

17 / 50

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

18 / 50

18. Which of the following liquids will show the highest decrease in viscosity with rise in temperature?

19 / 50

19. Which gas law explains why lungs may overexpand and rupture if a scuba diver ascends too quickly?

20 / 50

20. Why does honey flow more slowly than water?

21 / 50

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

22 / 50

22. Which of the following properties is common to both liquids and gases?

23 / 50

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

24 / 50

24. Which intermolecular force explains the higher boiling point of HF compared to HCl?

25 / 50

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

26 / 50

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

27 / 50

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

28 / 50

28. A mixture of gases contains 2 mol and 1 mol . If the total pressure is 9 atm, the partial pressure of helium is:

29 / 50

29. 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?

30 / 50

30. A 10 g sample of helium occupies 5.6 L at STP (273 K, 1 atm). Using ideal gas law, calculate molar mass of helium.

31 / 50

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

32 / 50

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

33 / 50

33. The relation between critical constants and van der Waals constants is:

34 / 50

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

35 / 50

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

36 / 50

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

37 / 50

37. Which of the following best describes the cause of deviation in van der Waals equation?

38 / 50

38. Which of the following liquids will have the highest vapour pressure at room temperature?

39 / 50

39. Which of the following best explains why gases are compressible but solids are not?

40 / 50

40. The graph of Boyle’s law (P vs V) at constant temperature is:

41 / 50

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

42 / 50

42. Which property enables gases to be stored in large amounts in small steel cylinders?

43 / 50

43. Which of the following substances lowers surface tension when added to water?

44 / 50

44. Which value of should be used when is in atm and in liters?

45 / 50

45. Which curve best represents isothermal compression of a gas?

46 / 50

46. Mountaineers experience breathing difficulties at high altitude mainly due to:

47 / 50

47. Why does a soft drink fizz more when opened at room temperature compared to when it is chilled?

48 / 50

48. Which of the following correctly represents enthalpy of sublimation ()?

49 / 50

49. Order the intermolecular forces from weakest to strongest:

50 / 50

50. Which phenomenon demonstrates surface tension in everyday life?

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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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