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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.

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  • Total Questions: 30
  • Time Allotted: 45 minutes
  • Passing Score: 50%
  • Randomization: Yes
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

Good luck! 👍

1 / 30

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

2 / 30

2. In Andrews’ CO₂ isotherm, what does the portion beyond the horizontal line (on further compression) represent?

3 / 30

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

4 / 30

4. Which of the following gases will have the same average kinetic energy at 300 K?

5 / 30

5. Which property best explains why iodine () has a higher melting point than fluorine ()?

6 / 30

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

7 / 30

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

8 / 30

8. Which gas law is most directly applied to explain the working of hot air balloons?

9 / 30

9. Under which conditions does best describe real gases?

10 / 30

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

11 / 30

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

12 / 30

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

13 / 30

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

14 / 30

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

15 / 30

15. Which application of surface tension is used in medicine?

16 / 30

16. 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?

17 / 30

17. In the pressure derivation, why is the factor included in the equation?

18 / 30

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

19 / 30

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

20 / 30

20. Viscosity of a liquid is defined as:

21 / 30

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

22 / 30

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

23 / 30

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

24 / 30

24. A gas cylinder contains 5.0 mol of O₂ and 3.0 mol of N₂ at 300 K in a 10 L container. Calculate the total pressure of the mixture using the ideal gas equation ().

25 / 30

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

26 / 30

26. Which of the following gases cannot be liquefied at room temperature (298 K) by applying pressure?

27 / 30

27. At STP, 1 mole of an ideal gas occupies:

28 / 30

28. 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:

29 / 30

29. Effusion of a gas refers to:

30 / 30

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

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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

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. The phenomenon of vapour pressure lowering is responsible for:

2 / 50

2. 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:

3 / 50

3. What causes dipole–dipole interaction strength to increase?

4 / 50

4. Which of the following decreases vapour pressure of a liquid?

5 / 50

5. A gas mixture contains 4 g of H₂ and 64 g of O₂ at 300 K in a 10 L container. Find the total pressure. ().

6 / 50

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

7 / 50

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

8 / 50

8. A mixture of H₂ and O₂ is allowed to diffuse through a porous plug. If mixture contains equal masses of both gases, what is the ratio of their diffusion rates?

9 / 50

9. According to kinetic theory, the average kinetic energy of a molecule of an ideal gas is:

10 / 50

10. A balloon has a volume of 2.5 L at 20°C. At what temperature will it occupy 5.0 L, assuming pressure is constant?

11 / 50

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

12 / 50

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

13 / 50

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

14 / 50

14. In an experiment, 100 mL of hydrogen diffuses in 25 seconds. How long will it take for the same volume of oxygen () to diffuse under identical conditions?

15 / 50

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

16 / 50

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

17 / 50

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

18 / 50

18. How many liters of nitrogen gas at STP contain molecules?

19 / 50

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

20 / 50

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

21 / 50

21. Order the intermolecular forces from weakest to strongest:

22 / 50

22. The diffusion rate of (M=28) compared to (M=44) is:

23 / 50

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

24 / 50

24. If for a gas, it means:

25 / 50

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

26 / 50

26. Surface tension decreases with:

27 / 50

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

28 / 50

28. A mixture of 2 mol , 3 mol , and 5 mol exerts 9 atm total pressure. The partial pressure of is:

29 / 50

29. Which factor does not directly affect viscosity of liquids?

30 / 50

30. Vapour pressure curves of volatile liquids intersect the atmospheric pressure line at:

31 / 50

31. 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 ?

32 / 50

32. Which factor explains why solid (dry ice) sublimes at room temperature?

33 / 50

33. 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.

34 / 50

34. At absolute zero (), the thermal energy of an ideal gas is:

35 / 50

35. Which of the following liquids has the highest viscosity at room temperature?

36 / 50

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

37 / 50

37. 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?

38 / 50

38. Which factor increases both melting and boiling points of a substance?

39 / 50

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

40 / 50

40. Which gas law relates pressure and volume at constant temperature?

41 / 50

41. At 100 °C, water boils because:

42 / 50

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

43 / 50

43. Which phenomenon demonstrates surface tension in everyday life?

44 / 50

44. Which assumption of kinetic theory accounts for the diffusion of gases?

45 / 50

45. The isotropic liquid phase differs from liquid crystal phases because:

46 / 50

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

47 / 50

47. What is the effect of decreasing temperature on molecular motion in a liquid?

48 / 50

48. 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?

49 / 50

49. If for a real gas, this means:

50 / 50

50. In liquids, compared to solids, molecules exhibit:

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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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