Exam-Style Online Test | Class 11 Chemistry: Thermodynamics
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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

Good luck! 👍

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 is meant by heat capacity of a substance?

2 / 30

2. Which of the following is a major application of the third law of thermodynamics?

3 / 30

3. If a system does no work but absorbs 250 J of heat, what is ?

4 / 30

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

5 / 30

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

6 / 30

6. Which of the following quantities is a state function related to the First Law?

7 / 30

7. The average bond enthalpy of O–H in H₂O is 463 kJ/mol. What is the total energy required to dissociate one mole of H₂O(g) into atoms?

8 / 30

8. Which of the following correctly describes spontaneity?

9 / 30

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

10 / 30

10. What is meant by molar heat capacity?

11 / 30

11. When one mole of ideal gas is heated at constant volume from to , the relation between and is:

12 / 30

12. In an open system, internal energy can change due to:

13 / 30

13. Which of the following is a real boundary?

14 / 30

14. Which of the following is the best example of an isolated system?

15 / 30

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

16 / 30

16. For a reaction where ΔH = +50 kJ and ΔS = +0.2 kJ/K, which statement is true?

17 / 30

17. Which statement correctly explains why ?

18 / 30

18. Which of the following represents a correct relation between state functions?

19 / 30

19. Why can the third law be used to determine absolute entropies experimentally?

20 / 30

20. Which of the following is true for entropy at absolute zero according to the third law?

21 / 30

21. Using formation enthalpies , , , compute for .

22 / 30

22. One mole of an ideal gas is heated in a closed, rigid container from to . What is the boundary work (W)?

23 / 30

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

24 / 30

24. In the first law of thermodynamics, the term q represents:

25 / 30

25. Hess’s law can be applied to find the enthalpy of formation of CH₄ from which data set?

26 / 30

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

27 / 30

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

28 / 30

28. Which of the following pairs includes only state functions?

29 / 30

29. 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 ?

30 / 30

30. The standard enthalpy of combustion of hydrogen is:

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

2 / 50

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

3 / 50

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

4 / 50

4. The rest of the universe excluding the system is called:

5 / 50

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

6 / 50

6. Which statement best summarizes Hess’s law?

7 / 50

7. What are extensive properties in thermodynamics?

8 / 50

8. What does Hess’s law state?

9 / 50

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

10 / 50

10. Which of the following represents a decrease in entropy?

11 / 50

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

12 / 50

12. What is meant by an adiabatic process?

13 / 50

13. Which of the following is true according to Hess’s law?

14 / 50

14. Two moles of an ideal gas are heated at constant pressure from 300 K to 500 K. If , what is the entropy change of the gas?

15 / 50

15. When a system releases 350 J of heat and has 150 J of work done on it, what is the change in internal energy?

16 / 50

16. For the combustion of methane, , calculate at 298 K.

17 / 50

17. What is the formula for Gibbs free energy?

18 / 50

18. The differential form of enthalpy is most generally written as:

19 / 50

19. For a gas compressed from 8.0 L to 3.0 L against an external pressure of 1.5 atm, what is the sign of work and its magnitude?

20 / 50

20. 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.

21 / 50

21. For an adiabatic process, what is the value of ( q )?

22 / 50

22. For a process with and , what will be the sign of ?

23 / 50

23. What is an intensive property in thermodynamics?

24 / 50

24. What is the correct mathematical expression for pressure–volume work done by a gas at constant external pressure?

25 / 50

25. Which of the following conditions leads to zero pressure–volume work?

26 / 50

26. In an open system, internal energy can change due to:

27 / 50

27. What happens to the internal energy of an ideal gas during an isothermal process?

28 / 50

28. The surface separating gas inside a balloon from the external air is a:

29 / 50

29. Using the data of question 385, if the initial temperature is 300 K, what is the final temperature?

30 / 50

30. Which of the following conditions must hold true for a process to be reversible?

31 / 50

31. The standard enthalpy of reaction can be expressed as:

32 / 50

32. The average bond enthalpy of O–H in H₂O is 463 kJ/mol. What is the total energy required to dissociate one mole of H₂O(g) into atoms?

33 / 50

33. Why is internal energy considered a state function, but work is not?

34 / 50

34. Which property remains intensive when two different liquids at the same temperature and pressure are carefully layered without mixing?

35 / 50

35. Which of the following pairs correctly shows both path functions?

36 / 50

36. Which of the following reactions can be used to illustrate Hess’s law?

37 / 50

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

38 / 50

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

39 / 50

39. Which of the following is an intensive property?

40 / 50

40. In the first law of thermodynamics, the term q represents:

41 / 50

41. The unit of pressure–volume work when expressed in SI units is:

42 / 50

42. What is meant by the heat of neutralization?

43 / 50

43. What are surroundings in thermodynamics?

44 / 50

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

45 / 50

45. A gas expands in a cylinder doing 400 J of work while losing 150 J of heat. What is ?

46 / 50

46. In a cyclic process where the system returns to its original state, which statement is true?

47 / 50

47. What is meant by lattice enthalpy?

48 / 50

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

49 / 50

49. The standard enthalpy of combustion of hydrogen is:

50 / 50

50. In an irreversible process, the total entropy change (system + surroundings) is always:

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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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