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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. Why is the discovery of critical constants important from Andrews’ experiments?

2 / 30

2. 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?

3 / 30

3. In the van der Waals equation, the constant accounts for:

4 / 30

4. If for a real gas at high pressure, the reason is:

5 / 30

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

6 / 30

6. Dalton’s law of partial pressures states that:

7 / 30

7. As pressure on a gas increases at constant temperature, what happens to molecular motion?

8 / 30

8. In a vs curve for a real gas, when the curve dips below the ideal line, it indicates:

9 / 30

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

10 / 30

10. Which gas shows the greatest deviation from ideal behavior?

11 / 30

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

12 / 30

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

13 / 30

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

14 / 30

14. Which real-world application relies on the temperature-sensitive color changes of cholesteric liquid crystals?

15 / 30

15. Which of the following graphs represents Charles’ law?

16 / 30

16. The average translational kinetic energy of one molecule of an ideal gas is given by:

17 / 30

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

18 / 30

18. The van der Waals equation for real gases is:

19 / 30

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

20 / 30

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

21 / 30

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

22 / 30

22. A sample of gas occupies 4.0 L at 2 atm pressure. What will be its volume at 1 atm, keeping temperature constant?

23 / 30

23. Which chemical process explains lowering of vapour pressure in salt water?

24 / 30

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

25 / 30

25. Which of the following statements is correct for Boyle’s law?

26 / 30

26. In the isotherms of CO₂ obtained by Andrews, the horizontal flat portion represents:

27 / 30

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

28 / 30

28. A gas exerts a pressure of 2.5 atm at 350 K. What will be its pressure at 175 K at constant volume?

29 / 30

29. Which real-life application illustrates Charles’ law?

30 / 30

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

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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 rate of diffusion of helium is how many times greater than that of methane (, M = 16)?

2 / 50

2. What volume will mol occupy at and ?

3 / 50

3. How does viscosity of a liquid change with temperature?

4 / 50

4. Two gases diffuse through a porous membrane. If H₂ diffuses 4 times faster than gas X, what is the molar mass of X?

5 / 50

5. Ammonia gas () diffuses through a porous pot in 40 s. How long would hydrogen () take under the same conditions?

6 / 50

6. Which factor does not affect the vapour pressure of a liquid?

7 / 50

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

8 / 50

8. Which of the following is assumed to remain constant during molecular collisions in kinetic theory?

9 / 50

9. In the kinetic theory of gases, the pressure exerted by a gas on the container walls is due to:

10 / 50

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

11 / 50

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

12 / 50

12. A mixture of H₂ and O₂ in a container has a total pressure of 2 atm. If the mole fraction of H₂ is 0.4, calculate partial pressures of both gases.

13 / 50

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

14 / 50

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

15 / 50

15. Which of the following gases shows larger deviation due to molecular volume rather than intermolecular attraction?

16 / 50

16. Surface tension of a liquid is defined as:

17 / 50

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

18 / 50

18. Which of the following applications is based on surface tension?

19 / 50

19. Which of the following gases will diffuse fastest at the same conditions?

20 / 50

20. A gas has mol in a rigid vessel at . What is in kPa?

21 / 50

21. Which of the following factors directly determines the thermal energy of a substance?

22 / 50

22. If the rms speed of oxygen molecules at 300 K is , what will be their rms speed at 1200 K?

23 / 50

23. Which of the following liquids has the highest vapour pressure at 25 °C?

24 / 50

24. Charles’ law can be explained using kinetic theory because:

25 / 50

25. A given gas occupies 200 mL at 740 mmHg. What volume will it occupy at 760 mmHg, assuming constant T?

26 / 50

26. At 100 °C, water boils because:

27 / 50

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

28 / 50

28. A gas has volume 6.0 L at 3 atm pressure. What will be its pressure if the volume changes to 2.0 L at constant temperature?

29 / 50

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

30 / 50

30. Which law relates viscous force to velocity gradient in liquids?

31 / 50

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

32 / 50

32. Which statement is true regarding London dispersion forces?

33 / 50

33. Which real-life example illustrates Avogadro’s law?

34 / 50

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

35 / 50

35. 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:

36 / 50

36. 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:

37 / 50

37. Which intermolecular force is primarily responsible for the liquefaction of nonpolar gases like and ?

38 / 50

38. When pressure on a solid increases, its melting point usually:

39 / 50

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

40 / 50

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

41 / 50

41. Which industrial application directly depends on control of viscosity?

42 / 50

42. Which of the following molecules exhibits dipole–dipole interactions?

43 / 50

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

44 / 50

44. Boyle’s law fails at:

45 / 50

45. 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?

46 / 50

46. Graham’s law of diffusion states that the rate of diffusion of a gas is:

47 / 50

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

48 / 50

48. A vessel contains 1 mol of O₂ and 2 mol of H₂ at 300 K. If total pressure = 9 atm, calculate the partial pressure of O₂.

49 / 50

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

50 / 50

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

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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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