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Class 11 Chemistry — Chapter 1: Some Basic Concepts of Chemistry Online Test

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Class 11 Chemistry: Some Basic Concepts of Chemistry 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. In the combustion of methane, , if 16 g CH₄ and 64 g O₂ are used, the limiting reagent is:

2 / 20

2. In the reaction , how many grams of AlCl₃ are produced from 54 g of Al?

3 / 20

3. In the reaction , how many moles of water are formed when 4 moles of hydrogen react with excess oxygen?

4 / 20

4. What mass of calcium carbonate is required to produce 44 g of CO₂ on decomposition? Reaction:

5 / 20

5. In the balanced combustion reaction of methane: , what is the coefficient of water?

6 / 20

6. Calculate the percentage of oxygen in water ().

7 / 20

7. In the synthesis of ammonia: , if 10 L of nitrogen is used, what volume of hydrogen is required at STP?

8 / 20

8. What is the atomicity of ammonium nitrate, ?

9 / 20

9. Determine the atomicity of (ammonium sulfate).

10 / 20

10. Which particle is directly rearranged during molecular chemical reactions?

11 / 20

11. Which of the following was a major merit of Dalton’s Atomic Theory?

12 / 20

12. Which of the following provides direct evidence for Avogadro’s Hypothesis?

13 / 20

13. In a closed system, 10 g of hydrogen reacts with 80 g of oxygen. What will be the total mass of water formed?

14 / 20

14. The Law of Definite Proportions states that:

15 / 20

15. According to the Law of Multiple Proportions, the ratios must always be:

16 / 20

16. In the reaction: the ratio of volumes of hydrogen, chlorine, and hydrogen chloride is:

17 / 20

17. What is the molecular mass of ?

18 / 20

18. The number is known as:

19 / 20

19. How many molecules of nitrogen gas are in 28 g of N₂?

20 / 20

20. What is the general formula for percentage composition of an element in a compound?

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Class 11 Chemistry: Some Basic Concepts of Chemistry 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. Why is it necessary to know the molecular mass when determining the molecular formula?

2 / 30

2. According to the Law of Conservation of Mass, in a chemical reaction:

3 / 30

3. Which statement is true regarding the Law of Definite Proportions?

4 / 30

4. Which merit of Dalton’s Atomic Theory connects directly with the development of the mole concept?

5 / 30

5. In NH₃, 14 g of nitrogen combines with 3 g of hydrogen. In H₂O, 16 g of oxygen combines with 2 g of hydrogen. If nitrogen and oxygen combine to form NO, the ratio of oxygen to nitrogen is:

6 / 30

6. One key merit of Dalton’s theory was that it provided:

7 / 30

7. Which example shows a variable composition compound that challenges Dalton’s fixed whole-number ratios?

8 / 30

8. In the reaction , 12 g Mg reacts with 16 g O₂. Which is limiting?

9 / 30

9. Which contribution of Dalton’s theory led to the calculation of relative atomic masses?

10 / 30

10. Calculate the percentage of hydrogen in water ().

11 / 30

11. What is meant by actual yield of a reaction?

12 / 30

12. In the balanced equation , what is the stoichiometric coefficient of oxygen?

13 / 30

13. Which is the correct molecular mass of ammonia ()?

14 / 30

14. Which of the following is the best definition of an atom?

15 / 30

15. What is the molecular mass of ?

16 / 30

16. The molecular formula of benzene is C₆H₆. Its empirical formula is:

17 / 30

17. Which of the following is a polyatomic molecule?

18 / 30

18. In , the percentage of chlorine is:

19 / 30

19. Dalton’s postulates emphasized that compounds are formed by:

20 / 30

20. What are the stoichiometric coefficients of reactants in the neutralization reaction ?

21 / 30

21. Which of the following provides direct evidence for Avogadro’s Hypothesis?

22 / 30

22. In the reaction of carbon monoxide and oxygen: , the volume ratio of CO : O₂ : CO₂ is:

23 / 30

23. Gay-Lussac’s law of gaseous volumes was one of the foundations for which later concept?

24 / 30

24. Which of the following represents a molecule and not a single atom?

25 / 30

25. Which compound is the main active ingredient in common painkillers like aspirin?

26 / 30

26. In the reaction , what is the stoichiometric coefficient of O₂?

27 / 30

27. Why is the atomic mass unit more convenient than grams in chemistry?

28 / 30

28. Dalton’s theory helped chemistry advance because it:

29 / 30

29. Which law explains why all gases occupy 22.4 L per mole at STP?

30 / 30

30. Which of the following pairs correctly shows “atom vs molecule”?

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Class 11 Chemistry: Some Basic Concepts of Chemistry 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. Dalton’s fixed-composition view of compounds is limited because some solids are non-stoichiometric. Which is a classic example?

2 / 50

2. Which of the following represents a molecule and not a single atom?

3 / 50

3. Which gas is responsible for the carbonation in soft drinks?

4 / 50

4. Which of the following is the first step in calculating percentage composition of a compound?

5 / 50

5. When 2 volumes of hydrogen combine with 1 volume of oxygen, the product formed is:

6 / 50

6. Which option correctly lists (monoatomic, diatomic, polyatomic) examples in order?

7 / 50

7. Which of the following correctly represents the atomicity of ozone?

8 / 50

8. Why are atoms considered neutral?

9 / 50

9. According to Avogadro’s Hypothesis, 22.4 L of any gas at STP contains:

10 / 50

10. For benzene (), what is the empirical formula?

11 / 50

11. Which environmental issue is directly related to chemical use of chlorofluorocarbons (CFCs)?

12 / 50

12. In the reaction , 12 g Mg reacts with 16 g O₂. Which is limiting?

13 / 50

13. Which statement about atomic mass unit is correct?

14 / 50

14. Which element pair and common element verify the Law of Reciprocal Proportions?

15 / 50

15. Which of the following best defines a molecule?

16 / 50

16. Who is credited with proposing the first modern atomic theory?

17 / 50

17. Which of the following is a molecule and not a compound?

18 / 50

18. The formula for percentage yield is:

19 / 50

19. The Law of Gaseous Volumes applies only to:

20 / 50

20. Which law explains why all gases occupy 22.4 L per mole at STP?

21 / 50

21. The molecular mass of (ethane) is:

22 / 50

22. Which property belongs to molecules but not to individual atoms?

23 / 50

23. Why was the concept of atomic mass unit (amu) introduced?

24 / 50

24. Which of the following best distinguishes an atom from a molecule?

25 / 50

25. According to the Law of Conservation of Mass, in a chemical reaction:

26 / 50

26. What is the relation between 1 mole of carbon-12 atoms and amu?

27 / 50

27. Which of the following is true about the mole concept?

28 / 50

28. If 10 g of CaCO₃ is decomposed, what volume of CO₂ at STP is theoretically produced? Reaction:

29 / 50

29. What volume will 3.5 moles of O₂ gas occupy at STP?

30 / 50

30. The study of enzymes acting as catalysts in biochemical reactions is an overlap of:

31 / 50

31. How many grams of CO₂ are produced when 44 g of propane () is completely burnt? Reaction:

32 / 50

32. Which particle is directly rearranged during molecular chemical reactions?

33 / 50

33. In the reaction , the theoretical yield is 36 g H₂O. If the actual yield is 30 g, what is the percentage yield?

34 / 50

34. Why was Avogadro’s Hypothesis initially rejected?

35 / 50

35. Dalton’s postulate that atoms are indestructible fails in which processes?

36 / 50

36. The molar volume of a gas at STP is:

37 / 50

37. Which of the following correctly explains why mass is conserved in chemical reactions?

38 / 50

38. A compound contains 80% carbon and 20% hydrogen by mass. What is its empirical formula?

39 / 50

39. What is the mass of carbon in 22 g of CO₂?

40 / 50

40. The empirical formula of a compound is NO₂ and its molecular mass is 92 g/mol. What is its molecular formula?

41 / 50

41. Which observation about isotopes exposes a limitation of Dalton’s “identical properties” postulate?

42 / 50

42. Why is percentage composition important in chemistry?

43 / 50

43. Why is molar mass important in stoichiometric calculations?

44 / 50

44. Which statement best summarizes Gay-Lussac’s Law of Gaseous Volumes?

45 / 50

45. In a neutralization reaction, 49 g of H₂SO₄ reacts with NaOH. How many grams of NaOH are required? Reaction:

46 / 50

46. Which of the following shows chemistry’s role in understanding the environment?

47 / 50

47. The Law of Conservation of Mass is not strictly valid in:

48 / 50

48. In , the percentage of chlorine is:

49 / 50

49. What is the relation between a molecular formula and an empirical formula?

50 / 50

50. Which of the following is true about molecules but not about atoms?

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Practice Some Basic Concepts of Chemistry MCQs
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Class 11 Chemistry: Chapter 1 — Some Basic Concepts of Chemistry Online Test

The Class 11 Chemistry: Chapter 1 – Some Basic Concepts of Chemistry Online Test provides a comprehensive pool of 394 MCQs designed to test and enhance your understanding of fundamental concepts in Chemistry. This test is free, CBSE/NCERT-aligned, and helps you assess your grasp on the key topics that form the foundation of the subject. With three difficulty levels, you can progressively challenge yourself and track your improvement over time.

What is this Chapter 1 Online Test?

This test contains three exam-style MCQ papers for Chapter 1: Some Basic Concepts of Chemistry:

  • 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 ~394 questions
  • Paper 3 (Hard) — Challenge: 50 questions · 75 min · Pass 70% · Randomized from the same pool + Certificate on pass

Note: Each paper is timed, auto-evaluated, and displays your score with answer reviews right after submission.

Topics covered in these online tests

In this test, you will practice essential topics from Chapter 1: Some Basic Concepts of Chemistry, which include:

  • Importance of Chemistry — Introduction to Chemistry, its relevance in real life and scientific advancements
  • Laws of Chemical Combination — Law of Mass Conservation, Law of Definite Proportions
  • Dalton’s Atomic Theory — Basic postulates, understanding atoms, and molecules
  • Mole Concept — Mole, Avogadro’s Number, Concept of Molar Mass, and Concept of Chemical Calculations
  • Molar Mass — Determining molar mass and its importance in chemical reactions
  • Percentage Composition — Calculation of percentage composition of compounds
  • Empirical & Molecular Formula — Concepts of empirical formula and molecular formula derivation
  • Stoichiometry — Concept of limiting reagent, and calculation of quantities involved in chemical reactions
  • Limiting Reagent — Importance in chemical reactions and stoichiometric calculations

How This Exam-Style Online Test Works

  • Pick a paper → Answer MCQs within time → Submit → Get instant score and answer review.
  • Timed MCQs: The test is timed, with Paper 1 being 30 minutes, Paper 2 being 45 minutes, and Paper 3 being 75 minutes.
  • Instant Feedback: After each paper, view your score along with a detailed summary and answer explanation.
  • Unlimited Retakes: You can retake the test as many times as you like, with fresh questions in Paper 2 and Paper 3.
  • Certificate: You will earn a certificate after passing Paper 3 with a score of 70% or more.

Who Can Take This Test?

  • Class 11 CBSE/NCERT students who are preparing for unit tests, mid-term exams, or final exams.
  • Students seeking to build a strong foundation in Chemistry for JEE/NEET or other competitive exams.
  • School students who need extra practice and want to assess their understanding of Chapter 1.
  • Teachers and tutors who want to provide students with extra practice and assess their skills.
  • Self-learners and home-schoolers who want a structured, easy-to-use resource to practice Chapter 1 topics.

Advantages of this Online Test

  • Real exam feel: Timed questions and instant feedback help you practice effectively under exam-like conditions.
  • Step-up difficulty: Start with easy questions in Paper 1, move to medium in Paper 2, and take the final challenge in Paper 3.
  • Unlimited attempts: Practice as many times as you like to perfect your skills and improve your score.
  • Completely free: No fees, no charges—just unlimited access to the online test.

How This Test Helps You Study Better

  • Step 1 – Concept Check: Take Paper 1 to check your understanding of basic concepts.
  • Step 2 – Reinforce Learning: Attempt Paper 2 for a mix of concept and numerical questions.
  • Step 3 – Challenge Yourself: Attempt Paper 3 to assess your readiness for exams.
  • Step 4 – Review: Carefully analyze your results and revisit concepts you missed.

Important Notes (Read Before You Start)

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