Exam-Style Online Test | Class 11 Chemistry: Thermodynamics

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. Which of the following compounds has the highest lattice enthalpy?

2 / 30

2. Which example best represents an open system?

3 / 30

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

4 / 30

4. Which of the following is not a correct example of a system?

5 / 30

5. Which statement correctly distinguishes standard conditions from STP in many textbooks?

6 / 30

6. When a hot metal rod is placed in cold water, heat transfer continues until:

7 / 30

7. Which statement about enthalpy is correct?

8 / 30

8. Which of the following is a path function?

9 / 30

9. For a monatomic ideal gas, if , what is ?

10 / 30

10. What is meant by the heat of atomization of an element or compound?

11 / 30

11. Why is the heat of neutralization nearly constant for all strong acid–strong base reactions?

12 / 30

12. Which of the following equations represents a heat of neutralization reaction?

13 / 30

13. Which of the following statements about absolute entropy is true?

14 / 30

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

15 / 30

15. The overall heat of solution (ΔHsol) can be expressed as:

16 / 30

16. For a reversible isothermal expansion of an ideal gas, which quantity depends on the process path?

17 / 30

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

18 / 30

18. Which of the following sets contains only intensive properties?

19 / 30

19. If the molar heat capacity of a monatomic ideal gas at constant volume is , what is its heat capacity at constant pressure?

20 / 30

20. Which thermodynamic function becomes zero at absolute zero for a perfect crystal?

21 / 30

21. What does the First Law of Thermodynamics state?

22 / 30

22. The standard heat of combustion of ethane (C₂H₆) is –1560 kJ mol⁻¹. What does the negative sign indicate?

23 / 30

23. For a solute A in solution, the standard chemical potential μ°A corresponds to which condition?

24 / 30

24. If , which condition indicates a spontaneous process?

25 / 30

25. If a chemical equation is multiplied by a factor n, then according to Hess’s law, ΔH becomes:

26 / 30

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

27 / 30

27. Which of the following characteristics does not apply to an open system?

28 / 30

28. A reaction is endothermic but spontaneous at room temperature. What does this suggest about ΔS?

29 / 30

29. Which of the following statements about isolated systems is incorrect?

30 / 30

30. For an endothermic process to be spontaneous, what must be true?

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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. In a closed system, 500 J of heat is supplied and the system does 200 J of work on the surroundings. What is ?

2 / 50

2. For a solute A in solution, the standard chemical potential μ°A corresponds to which condition?

3 / 50

3. What is meant by molar heat capacity?

4 / 50

4. Why is Gibbs free energy an important thermodynamic function?

5 / 50

5. Which pair below includes only state functions?

6 / 50

6. What is an isolated system in thermodynamics?

7 / 50

7. Which setup is the best example of a closed system?

8 / 50

8. If ΔH₁ = –393.5 kJ and ΔH₂ = –283 kJ, what is ΔH for the reaction C(s) + ½O₂(g) → CO(g)?

9 / 50

9. Which of the following statements is true about spontaneous processes?

10 / 50

10. When work is done on the system by the surroundings, its sign according to the chemistry convention is:

11 / 50

11. What is an imaginary boundary in thermodynamics?

12 / 50

12. Which property is necessarily constant for any closed system undergoing any process?

13 / 50

13. How can the absolute entropy of a substance at any temperature be calculated using the third law?

14 / 50

14. Which of the following correctly represents the relationship between enthalpy and internal energy?

15 / 50

15. Which of the following correctly expresses the difference between molar heat capacities and ?

16 / 50

16. According to the third law, what is the entropy of an imperfect crystal at 0 K?

17 / 50

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

18 / 50

18. Which example best represents an open system?

19 / 50

19. Which of the following correctly describes an isothermal expansion of an ideal gas?

20 / 50

20. The standard enthalpy of combustion is defined as:

21 / 50

21. Which of the following processes is spontaneous at high temperatures but not at low temperatures?

22 / 50

22. If 500 J of heat raises the temperature of a metal block by 10 K, what is its heat capacity?

23 / 50

23. What does the term pressure–volume (P–V) work represent in thermodynamics?

24 / 50

24. The overall heat of solution (ΔHsol) can be expressed as:

25 / 50

25. In thermodynamics, the earth’s atmosphere can be regarded as:

26 / 50

26. An ideal gas has . What are and for the gas?

27 / 50

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

28 / 50

28. For the same volume change, how does entropy change differ between reversible and irreversible expansion of a gas?

29 / 50

29. The SI unit of heat energy is:

30 / 50

30. The process of dissolving anhydrous CuSO₄ in water is accompanied by:

31 / 50

31. The enthalpy of decomposition of CaCO₃(s) → CaO(s) + CO₂(g) can be calculated using Hess’s law by combining:

32 / 50

32. Why is it impossible to reach absolute zero temperature?

33 / 50

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

34 / 50

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

35 / 50

35. Which of the following best describes Gibbs free energy?

36 / 50

36. What is true for a system undergoing a spontaneous process at constant temperature and pressure?

37 / 50

37. The equation is valid for:

38 / 50

38. Which of the following pairs contains only extensive properties?

39 / 50

39. Which of the following is the correct expression of Hess’s law?

40 / 50

40. Which of the following equations correctly represents the standard enthalpy of formation of ammonia?

41 / 50

41. Which of the following characteristics does not apply to an open system?

42 / 50

42. What does the term ( TS ) represent in the Gibbs free energy equation?

43 / 50

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

44 / 50

44. For a process with ΔH = –200 kJ and ΔS = –0.3 kJ/K, when is the process spontaneous?

45 / 50

45. How can the third law be applied to determine the feasibility of a reaction?

46 / 50

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

47 / 50

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

48 / 50

48. Which statement correctly explains the First Law of Thermodynamics?

49 / 50

49. If the molar heat capacity of a monatomic ideal gas at constant volume is , what is its heat capacity at constant pressure?

50 / 50

50. What does the First Law of Thermodynamics state?

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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)

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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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