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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. If the pressure of a fixed mass of gas is plotted against its reciprocal of volume (1/V), the graph is:

2 / 30

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

3 / 30

3. The critical volume () refers to:

4 / 30

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

5 / 30

5. Why do real gases deviate from ideal behavior at low temperature?

6 / 30

6. Why do real gases deviate from ideal behavior at high pressure?

7 / 30

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

8 / 30

8. The reason noble gases show an increasing trend in boiling point down the group is:

9 / 30

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

10 / 30

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

11 / 30

11. Which of the following liquids shows the strongest intermolecular forces?

12 / 30

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

13 / 30

13. The helical arrangement of molecules in cholesteric (chiral nematic) liquid crystals leads to:

14 / 30

14. Why does kinetic theory assume intermolecular forces are negligible in gases?

15 / 30

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

16 / 30

16. A 5 L container has a mixture of 2 mol of O₂ and 3 mol of N₂ at 300 K. Calculate the total pressure of the gas mixture. ( L·atm·K⁻¹·mol⁻¹)

17 / 30

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

18 / 30

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

19 / 30

19. Effusion of a gas refers to:

20 / 30

20. Unit of viscosity in the CGS system is:

21 / 30

21. According to kinetic theory, pressure of a gas arises due to:

22 / 30

22. Which real-life application is based on the concept of viscosity?

23 / 30

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

24 / 30

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

25 / 30

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

26 / 30

26. Which critical constants of CO₂ make it easy to use as a supercritical fluid?

27 / 30

27. 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?

28 / 30

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

29 / 30

29. 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:

30 / 30

30. 200 mL of H₂ at 27 °C and 1 atm is mixed with 200 mL of O₂ at 27 °C and 2 atm. The final pressure in 400 mL vessel at 27 °C will be:

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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. A 5 g sample of an unknown gas occupies 2 L at 1 atm and 300 K. Calculate its molar mass.

2 / 50

2. Which equation best describes the boundary between liquid and supercritical fluid?

3 / 50

3. Which equation represents the ideal gas law?

4 / 50

4. Which of the following states of matter has the highest degree of random molecular motion?

5 / 50

5. Which of the following increases with addition of surfactants in water?

6 / 50

6. In the above mixture (Q471), what is the partial pressure of N₂?

7 / 50

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

8 / 50

8. Two gases are mixed into a final vessel at . Gas A: at . Gas B: at . Assuming ideal behavior, what is the final total pressure at ?

9 / 50

9. Unit of viscosity in the CGS system is:

10 / 50

10. 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.

11 / 50

11. Which gas can be liquefied more easily due to stronger London dispersion forces?

12 / 50

12. Surface tension becomes zero at:

13 / 50

13. Why do nonpolar molecules with larger molar mass generally have higher boiling points than smaller nonpolar molecules?

14 / 50

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

15 / 50

15. According to kinetic theory, pressure of a gas arises due to:

16 / 50

16. Which real-life application is based on the concept of viscosity?

17 / 50

17. Which condition favors gaseous state most strongly?

18 / 50

18. Which of the following best describes the nematic liquid crystal phase?

19 / 50

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

20 / 50

20. Supercritical CO₂ is used in green chemistry because:

21 / 50

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

22 / 50

22. Why does carbon dioxide show greater deviation than nitrogen at the same conditions?

23 / 50

23. Which of the following best explains why detergents help in cleaning greasy clothes?

24 / 50

24. Which pair of gases will diffuse at approximately the same rate?

25 / 50

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

26 / 50

26. The ratio of diffusion rates of NH₃ (M = 17) and HCl (M = 36.5) is approximately:

27 / 50

27. Which type of intermolecular force exists in all substances, regardless of polarity?

28 / 50

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

29 / 50

29. The critical volume () is:

30 / 50

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

31 / 50

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

32 / 50

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

33 / 50

33. A steel cylinder contains oxygen gas at 10 atm and 300 K. If the cylinder is heated to 600 K without changing volume, what will be the new pressure?

34 / 50

34. For a gas at constant temperature, when volume decreases by half, pressure:

35 / 50

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

36 / 50

36. Which change of state explains the working of solid air fresheners (naphthalene balls)?

37 / 50

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

38 / 50

38. Which of the following is the correct dimension of the term in the pressure equation?

39 / 50

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

40 / 50

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

41 / 50

41. In the compressibility curve of hydrogen and helium, the value is always:

42 / 50

42. In the nematic phase of liquid crystals, molecules are:

43 / 50

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

44 / 50

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

45 / 50

45. Which is the main cause of deviation of real gases from ideal behavior at low temperature?

46 / 50

46. Which law is applied when calculating the pressure exerted by different gases in a scuba tank mixture (oxygen + nitrogen)?

47 / 50

47. Why is critical temperature important in liquefaction of gases?

48 / 50

48. The root mean square (RMS) speed is defined as:

49 / 50

49. Which of the following mathematical forms correctly represents Boyle’s law?

50 / 50

50. When ammonia and hydrogen chloride gases diffuse toward each other, a white ring of forms closer to HCl because:

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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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