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. For a diatomic ideal gas, . What is ?

2 / 30

2. What is the standard enthalpy of formation (ΔH°f) of an element in its most stable form?

3 / 30

3. Which of the following has the greatest increase in entropy?

4 / 30

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

5 / 30

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

6 / 30

6. Under standard conditions, what is the activity assumed for a 1 M ideal solute?

7 / 30

7. If a system is divided into two equal halves, what happens to its total energy, assuming no interaction between the halves?

8 / 30

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

9 / 30

9. Which equation links the ratio of heat capacities (γ) with adiabatic processes?

10 / 30

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

11 / 30

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

12 / 30

12. What is a reversible process in thermodynamics?

13 / 30

13. Which of the following changes leads to an increase in entropy?

14 / 30

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

15 / 30

15. A closed system is one in which:

16 / 30

16. Which of the following is the best example of an open system?

17 / 30

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

18 / 30

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

19 / 30

19. Which example best represents an open system?

20 / 30

20. When a system does 250 J of work on surroundings and absorbs 150 J of heat, what is the change in its internal energy?

21 / 30

21. 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?

22 / 30

22. In a reaction where Δn = 0 (no change in moles of gas), what can be said about ΔH and ΔU?

23 / 30

23. What is meant by a spontaneous process?

24 / 30

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

25 / 30

25. Why are standard conditions specified when tabulating thermodynamic data?

26 / 30

26. Which of the following correctly represents the average bond enthalpy of C–H bonds in methane?

27 / 30

27. Which of the following substances will have the highest heat of combustion per mole?

28 / 30

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

29 / 30

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

30 / 30

30. What is meant by the heat of dilution?

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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. One mole of an ideal gas expands isothermally and reversibly at 298 K from 2.0 L to 8.0 L. What is of the gas?

2 / 50

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

3 / 50

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

4 / 50

4. For an ideal gas, which statement best describes the relation between ΔH and ΔU?

5 / 50

5. When will a reaction with and be spontaneous?

6 / 50

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

7 / 50

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

8 / 50

8. What type of work is associated with the expansion of a gas?

9 / 50

9. Which of the following is not a state function?

10 / 50

10. For a reaction with and , the process will be spontaneous when:

11 / 50

11. What is meant by a boundary in thermodynamics?

12 / 50

12. In an isothermal reversible expansion of an ideal gas, the entropy change of the system is:

13 / 50

13. Why are industrial chemical reactors considered open systems?

14 / 50

14. What is meant by the heat of dilution?

15 / 50

15. Which example best represents an open system?

16 / 50

16. What is the thermodynamic definition of enthalpy H?

17 / 50

17. Which of the following processes involves heat transfer but no work done?

18 / 50

18. Which of the following is an example of work done by a thermodynamic system?

19 / 50

19. For a closed system at constant pressure, the heat exchanged is related to enthalpy by which expression?

20 / 50

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

21 / 50

21. Which of the following is an important use of Hess’s law?

22 / 50

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

23 / 50

23. Which of the following conditions makes a process irreversible?

24 / 50

24. Which property cannot be determined without the third law of thermodynamics?

25 / 50

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

26 / 50

26. Using formation enthalpies , , , compute for .

27 / 50

27. What is meant by the heat of neutralization?

28 / 50

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

29 / 50

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

30 / 50

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

31 / 50

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

32 / 50

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

33 / 50

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

34 / 50

34. If a system is divided into two equal halves, what happens to its total energy, assuming no interaction between the halves?

35 / 50

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

36 / 50

36. Which of the following is an extensive property?

37 / 50

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

38 / 50

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

39 / 50

39. What is meant by the standard enthalpy of a reaction (ΔH°rxn)?

40 / 50

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

41 / 50

41. Which combination of ΔH and ΔS values always gives a non-spontaneous reaction?

42 / 50

42. In thermodynamics, what is meant by heat?

43 / 50

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

44 / 50

44. In thermodynamics, what are state variables?

45 / 50

45. What is the SI unit of heat capacity?

46 / 50

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

47 / 50

47. In thermodynamics, what does the term "work" refer to?

48 / 50

48. What does the symbol ( G ) represent in thermodynamics?

49 / 50

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

50 / 50

50. A reaction at 1 atm releases 250 kJ of heat as measured by a coffee-cup calorimeter. What is for the reaction?

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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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