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Class 11 Chemistry — Chapter 6: Thermodynamics Online Test

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Class 11 Chemistry: Thermodynamics 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

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1 / 20

1. Using formation enthalpies , , , compute for .

2 / 20

2. One mole of an ideal gas expands isothermally and reversibly at 300 K from 5.0 L to 15.0 L. What is the work done by the gas?

3 / 20

3. The second law of thermodynamics can be expressed in terms of entropy as:

4 / 20

4. Which condition represents equilibrium between spontaneous and non-spontaneous behavior?

5 / 20

5. Which of the following statements is correct about average bond enthalpy?

6 / 20

6. The enthalpy of formation of CO₂ is –393.5 kJ/mol and that of CO is –110.5 kJ/mol. What is the enthalpy change for oxidation of CO to CO₂?

7 / 20

7. For the reaction , the heat of neutralization is approximately:

8 / 20

8. If for air, what is ?

9 / 20

9. What is the difference between specific heat capacity and molar heat capacity?

10 / 20

10. Which statement about enthalpy is correct?

11 / 20

11. Which pair below includes only state functions?

12 / 20

12. Which of the following correctly differentiates extensive from intensive properties?

13 / 20

13. During the compression of a gas in a closed cylinder, which of the following statements is true?

14 / 20

14. In thermodynamics, which statement about a closed system is always true?

15 / 20

15. In an isothermal process, which of the following remains constant?

16 / 20

16. In thermodynamics, what are state variables?

17 / 20

17. In the equation , a negative value of ( w ) indicates that:

18 / 20

18. When a system absorbs heat, the sign of q according to chemistry convention is:

19 / 20

19. In the equation , what does each term represent?

20 / 20

20. Consider the reaction: . The standard enthalpy of formation of water is –286 kJ mol⁻¹. What is ΔH°rxn?

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Class 11 Chemistry: Thermodynamics 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. What does the symbol ( G ) represent in thermodynamics?

2 / 30

2. Why does the absolute entropy of a perfect crystal become zero at 0 K?

3 / 30

3. Hess’s law is based on which fundamental concept?

4 / 30

4. Why is internal energy considered an extensive property?

5 / 30

5. Which of the following equations represents an adiabatic process?

6 / 30

6. Which of the following is an example where an imaginary boundary is most useful?

7 / 30

7. What is meant by the heat of dilution?

8 / 30

8. What is meant by a state function in thermodynamics?

9 / 30

9. What does Hess’s law state?

10 / 30

10. Which of the following correctly expresses the entropy at 0 K for a perfect crystal?

11 / 30

11. A standard Gibbs energy change ΔG° is most directly related to which equilibrium quantity at 298 K?

12 / 30

12. One mole of an ideal gas expands isothermally and reversibly at 300 K from 5.0 L to 15.0 L. What is the work done by the gas?

13 / 30

13. The third law of thermodynamics provides a method to determine which of the following?

14 / 30

14. What is the expression for entropy change (ΔS) in a reversible process?

15 / 30

15. When will a reaction with and be spontaneous?

16 / 30

16. If , which of the following statements must be true?

17 / 30

17. If ΔH = –100 kJ and ΔS = +200 J/K, at what temperature does the reaction become spontaneous?

18 / 30

18. Which of the following systems has zero entropy at 0 K according to the third law of thermodynamics?

19 / 30

19. What does the third law of thermodynamics state?

20 / 30

20. The enthalpy of formation of CO(g) can be calculated using Hess’s law from:

21 / 30

21. For a reaction with and , above what temperature will it be spontaneous?

22 / 30

22. For an ideal gas with at 300 K, what is and ?

23 / 30

23. A closed system with adiabatic walls is compressed so that 800 J of work is done on the system. The heat transfer is zero. What is ?

24 / 30

24. Which factor affects the bond enthalpy of a molecule?

25 / 30

25. Which of the following statements about P–V work is true?

26 / 30

26. Why do polyatomic molecules have average bond enthalpies instead of specific ones?

27 / 30

27. What does a high bond enthalpy value indicate about a molecule?

28 / 30

28. Gibbs free energy (G) is useful because it indicates:

29 / 30

29. If , which condition indicates a spontaneous process?

30 / 30

30. At constant volume, the molar heat capacity of an ideal gas is represented as:

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Class 11 Chemistry: Thermodynamics 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. Which of the following quantities is not a state function?

2 / 50

2. Consider the reaction: . The standard enthalpy of formation of water is –286 kJ mol⁻¹. What is ΔH°rxn?

3 / 50

3. Which of the following is a non-spontaneous process?

4 / 50

4. Which of the following reactions has ΔH° = 0 by definition?

5 / 50

5. One mole of an ideal gas undergoes isothermal, reversible compression at 300 K from 10.0 L to 2.0 L. Compute the work on the gas.

6 / 50

6. For a pure liquid, density is classified as which type of property?

7 / 50

7. What is the fundamental relation between molar heat capacities at constant pressure and volume for an ideal gas?

8 / 50

8. The heat of atomization of chlorine gas (Cl₂) is 243 kJ/mol. What is the bond dissociation energy of the Cl–Cl bond?

9 / 50

9. Which condition must be satisfied for a system to be considered isolated?

10 / 50

10. Under which conditions does Gibbs free energy remain constant?

11 / 50

11. What is meant by heat capacity of a substance?

12 / 50

12. Hess’s law can also be applied in determining which other thermodynamic function besides ΔH?

13 / 50

13. Which factor affects the bond enthalpy of a molecule?

14 / 50

14. The standard heat of formation of any element in its most stable form is:

15 / 50

15. The standard enthalpy of combustion of hydrogen is:

16 / 50

16. For a diatomic ideal gas, . What is ?

17 / 50

17. Why is greater than for gases?

18 / 50

18. For an ideal gas, the relation between molar heat capacities and is:

19 / 50

19. If a chemical reaction has ΔH = –150 kJ and ΔS = +0.1 kJ/K, what will be the sign of ΔG at 298 K?

20 / 50

20. In an isothermal process, which of the following remains constant?

21 / 50

21. Which of the following is an irreversible process?

22 / 50

22. What happens to the entropy of all pure crystalline solids at 0 K according to the third law?

23 / 50

23. For an ideal gas undergoing an isothermal process, which statement is correct?

24 / 50

24. Why does the absolute entropy of a perfect crystal become zero at 0 K?

25 / 50

25. Why is Hess’s law particularly useful in thermochemistry?

26 / 50

26. Which of the following correctly describes a non-spontaneous process?

27 / 50

27. Which of the following quantities is a state function?

28 / 50

28. The enthalpy of formation of CO(g) can be calculated using Hess’s law from:

29 / 50

29. What does a positive value of indicate about a process?

30 / 50

30. For the neutralization between a weak acid and strong base, the heat of neutralization is less than –57.1 kJ mol⁻¹ because:

31 / 50

31. At 298 K, the equilibrium constant for a reaction is . What is ?

32 / 50

32. What is meant by the standard heat of formation (ΔH°f)?

33 / 50

33. Which of the following statements correctly describes entropy?

34 / 50

34. The SI unit of heat energy is:

35 / 50

35. Which of the following statements correctly describes work in thermodynamics?

36 / 50

36. A perfectly insulated and sealed container of gas is an example of which system?

37 / 50

37. What is meant by the heat of combustion of a substance?

38 / 50

38. During compression, work is done on the gas by surroundings. What is the sign of ( w ) in ?

39 / 50

39. What is meant by lattice enthalpy?

40 / 50

40. What does the equation represent?

41 / 50

41. What is the general thermodynamic criterion for spontaneity of a process at constant temperature and pressure?

42 / 50

42. What happens to the heat of dilution as a solution becomes very dilute?

43 / 50

43. What is meant by an adiabatic process?

44 / 50

44. When concentrated sulfuric acid is diluted with water, the process is highly exothermic. What safety precaution should be followed?

45 / 50

45. What is an intensive property in thermodynamics?

46 / 50

46. What does the superscript “°” in ΔH° or ΔG° signify?

47 / 50

47. Which statement best explains the relationship between lattice enthalpy and ionic stability?

48 / 50

48. Which of the following represents the standard heat of formation of water?

49 / 50

49. Hess’s law helps to determine which of the following?

50 / 50

50. In a gas cylinder with a movable piston, the piston surface acts as which type of boundary?

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Practice Thermodynamics MCQs
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Class 11 Chemistry — Chapter 6: Thermodynamics Online Test

The Class 11 Chemistry: Chapter 6 – Thermodynamics Online Test provides a comprehensive pool of 395 MCQs designed to evaluate your understanding of the core principles of thermodynamics. This test is free, aligned with the NCERT/CBSE Class 11 syllabus, and offers unlimited practice opportunities to help you master thermodynamic concepts. With three levels of difficulty, you can gradually increase the challenge and track your progress.

Whether you are preparing for school exams or competitive tests like JEE/NEET, this online test will guide you through the key concepts of thermodynamics, from energy conservation to the laws governing thermodynamic processes. This test works as both a revision tool and a mock exam to enhance your speed, accuracy, and conceptual clarity.

Feeling a bit anxious before your exams? Don’t worry, this page is here to help. It’s like a mock test for you to practice at your own pace—whether at home or on the go. With each attempt, you’ll see your score, get instant feedback, and learn from the mistakes. When you’re ready, challenge yourself with Paper 3 for a higher level of difficulty and earn a certificate.

What is the Class 11 Chemistry: Thermodynamics Online Test?

This page contains three exam-style MCQ papers for Chapter 6: Thermodynamics:

  • 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 ~395 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, ensuring a new set of questions on each attempt. All papers are timed, auto-evaluated, and show your score with detailed answer reviews.

Topics Covered in this Online Test

This online test covers a wide range of topics in Thermodynamics from the NCERT Class 11 Chemistry syllabus. The following topics are included:

  • Introduction to Thermodynamics — Definition, system, surroundings, and types of systems
  • First Law of Thermodynamics — Internal energy, heat, work, and the concept of energy conservation
  • Enthalpy — Enthalpy changes, heat capacity, and Hess’s Law
  • Work and Heat — Types of work, heat exchange in different processes (isothermal, adiabatic)
  • Thermodynamic Processes — Isothermal, adiabatic, isobaric, isochoric processes
  • Second Law of Thermodynamics — Entropy, spontaneous processes, and reversibility
  • Gibbs Free Energy — Criteria for spontaneity, Gibbs free energy change (ΔG)
  • Heat Engines and Refrigerators — Carnot engine, efficiency, and refrigerator working
  • Entropy and its significance — Entropy as a measure of disorder, Clausius inequality
  • Thermodynamic Cycles — Carnot cycle, Rankine cycle, efficiency of cycles

For a more detailed understanding, you can refer to: Thermodynamics MCQs and explore more questions from Class 11 Chemistry MCQ Collection.

How This Exam-Style Online Test Works

Quick Summary: Select a paper → answer MCQs within the given time → submit → instantly see your score and review your answers. Achieve a passing score on Paper 3 to earn a certificate.

What you’ll see during the test

  • MCQs: One question with four options (A, B, C, D).
  • Timer on top: P1: 30 min • P2: 45 min • P3: 75 min.
  • Pagination: Typically 10 questions per page (navigate through using page controls).
  • Navigation: Use Next/Prev buttons or the question map to revisit questions before submission.
  • View Result: After submitting, click View Result to see your score, correct answers, and mistakes.
  • Restart: Click Restart Test to retry and improve your score with a fresh set of questions (Paper 2 & Paper 3).

Note: After completing the test, feel free to share your feedback on the result page.

Marking & pass criteria

  • Scoring: +1 for correct answers, 0 for incorrect answers (no negative marking).
  • Passing marks: Paper 1 — 40%, Paper 2 — 50%, Paper 3 — 70%.
  • Randomization: Paper 2 and Paper 3 shuffle questions from a large question pool, so every attempt offers fresh challenges.

Who can take this test?

  • Class 11 CBSE students preparing for midterms, unit tests, or final exams in Chemistry.
  • NEET and JEE aspirants strengthening their understanding of thermodynamics and core concepts.
  • Self-learners and home-schoolers looking for a structured way to practice thermodynamics.
  • Teachers and tutors seeking pre-made assessments for students to test their knowledge.
  • Other boards & countries following similar Chemistry curriculums.

Benefits of this Online Test

  • Real exam experience: Timed MCQs simulate exam conditions, building speed and accuracy.
  • Instant results: See your score right away and review the answers for better understanding.
  • Step-up difficulty: Progress through Paper 1 → Paper 2 → Paper 3 and earn a certificate.
  • Unlimited practice: Practice as many times as you need with randomized questions in Paper 2 & 3.
  • Completely free: No fees, no login required—just unlimited access to test your knowledge.

How This Test Helps You Study More Effectively

  • Step 1 – Concept Check: Start with Paper 1 to check your basic understanding.
  • Step 2 – Reinforcement: Attempt Paper 2 to reinforce your concepts.
  • Step 3 – Challenge: Finish with Paper 3 to test your exam readiness.
  • Step 4 – Review: Examine mistakes, understand explanations, and reattempt missed questions.
  • Step 5 – Retake Smartly: Reattempt after 1–2 days to ensure long-term retention and recall.

Important Notes (Please Read Before You Start)

  • Do not refresh or close the browser tab during the test to avoid session loss.
  • Best experience: Use a stable internet connection and the latest browser version (e.g., Chrome or Edge).
  • Allow cookies / local storage to track your progress and test session.
  • Safety: This test is 100% free—ignore any unsolicited payment requests.

More Practice for Class 11 Chemistry

After completing this online test, continue practicing with our comprehensive set of MCQs for other chapters: Class 11 Chemistry MCQs or practice other chapters from: Class 11 Chemistry Online Test Index.

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