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

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 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?

2 / 30

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

3 / 30

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

4 / 30

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

5 / 30

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

6 / 30

6. Why is the bond enthalpy of O=O lower than that of N≡N?

7 / 30

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

8 / 30

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

9 / 30

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

10 / 30

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

11 / 30

11. Which of the following processes occurs in an open system?

12 / 30

12. 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?

13 / 30

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

14 / 30

14. What does the term "thermodynamics" literally mean?

15 / 30

15. What is the SI unit of heat capacity?

16 / 30

16. If , which condition indicates a spontaneous process?

17 / 30

17. Which thermodynamic law is directly demonstrated by an isolated system?

18 / 30

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

19 / 30

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

20 / 30

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

21 / 30

21. A system defined by an imaginary boundary is often used when:

22 / 30

22. During expansion, a gas performs 300 J of work against constant external pressure. What happens to the system’s internal energy if no heat is supplied?

23 / 30

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

24 / 30

24. Which of the following statements about entropy in reversible and irreversible processes is correct?

25 / 30

25. What is the general relation between enthalpy change (ΔH) and internal energy change (ΔU)?

26 / 30

26. For a chemical reaction involving gases, which equation relates ΔH and ΔU?

27 / 30

27. Which of the following equations relates Gibbs free energy to maximum work?

28 / 30

28. Which of the following is an example of a spontaneous process?

29 / 30

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

30 / 30

30. Which of the following is an extensive property?

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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 systems has zero entropy at 0 K according to the third law of thermodynamics?

2 / 50

2. What is enthalpy (H) defined as in thermodynamics?

3 / 50

3. A human body can be considered as which type of system?

4 / 50

4. For a gas expansion where the system does 200 J of work and absorbs 500 J of heat, what is ?

5 / 50

5. What is meant by the term heat of hydration?

6 / 50

6. What is meant by the heat of neutralization?

7 / 50

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

8 / 50

8. What is meant by molar heat capacity?

9 / 50

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

10 / 50

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

11 / 50

11. Which of the following best defines the system in thermodynamics?

12 / 50

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

13 / 50

13. What does the First Law of Thermodynamics state?

14 / 50

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

15 / 50

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

16 / 50

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

17 / 50

17. 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?

18 / 50

18. Internal energy (U) is considered a state function because:

19 / 50

19. If the ΔH°f for CO₂(g) is –393.5 kJ/mol and for H₂O(l) is –286 kJ/mol, what is ΔH°rxn for combustion of CH₄(g)?

20 / 50

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

21 / 50

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

22 / 50

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

23 / 50

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

24 / 50

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

25 / 50

25. 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?

26 / 50

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

27 / 50

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

28 / 50

28. A sealed metal container of gas is heated on a flame. Which description fits the boundary and transfers?

29 / 50

29. Which of the following processes represents heat of atomization?

30 / 50

30. Which of the following statements is correct about system and surroundings?

31 / 50

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

32 / 50

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

33 / 50

33. Which of the following is an extensive property?

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

36 / 50

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

37 / 50

37. Which device operates based primarily on heat transfer between two bodies?

38 / 50

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

39 / 50

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

40 / 50

40. Why are industrial chemical reactors considered open systems?

41 / 50

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

42 / 50

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

43 / 50

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

44 / 50

44. Why is the N≡N bond in nitrogen gas so stable?

45 / 50

45. For a reaction in which the number of moles of gas decreases, what is the relation between ΔH and ΔU?

46 / 50

46. What is the general relation between enthalpy change (ΔH) and internal energy change (ΔU)?

47 / 50

47. When ΔG = 0, what does it signify?

48 / 50

48. What is an isolated system in thermodynamics?

49 / 50

49. What is the entropy change of the universe for an irreversible process?

50 / 50

50. What is the formula for Gibbs free energy?

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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).
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  • 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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