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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. In CO and CO₂, 12 g of carbon combines with 16 g and 32 g of oxygen, respectively. The ratio of masses of oxygen combining with the same mass of carbon is:

2 / 30

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

3 / 30

3. Which observation directly contradicts Dalton’s claim that “atoms of the same element are identical in mass and properties”?

4 / 30

4. What is the mass of calcium present in 50 g of calcium carbonate ()?

5 / 30

5. The average atomic mass of lithium is 6.94 u. Which isotopes contribute to this value?

6 / 30

6. Which postulate forms the basis of the Law of Definite Proportions?

7 / 30

7. Which of the following is true about the relation between mole, mass, and volume?

8 / 30

8. The stoichiometric coefficients of reactants in the balanced equation are:

9 / 30

9. Which of the following statements from Dalton’s theory is still valid today?

10 / 30

10. Calculate the percentage of oxygen in calcium carbonate ().

11 / 30

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

12 / 30

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

13 / 30

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

14 / 30

14. Which chemical is commonly used as an octane booster in fuels?

15 / 30

15. One mole of sodium chloride (NaCl) contains how many ions?

16 / 30

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

17 / 30

17. Which chemical is used in the agriculture industry as a pesticide?

18 / 30

18. Which atmospheric process is explained through chemistry?

19 / 30

19. Which statement is correct about monoatomic molecules?

20 / 30

20. Who is credited with introducing the concept of the “mole” in chemistry?

21 / 30

21. Which of the following is an example of an empirical formula?

22 / 30

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

23 / 30

23. In the combustion of 16 g of CH₄, what is the theoretical yield of CO₂? Reaction:

24 / 30

24. Which of the following compounds has the same molecular and empirical formula?

25 / 30

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

26 / 30

26. The number of oxygen atoms in 18 g of water is:

27 / 30

27. Which compound has the molar mass of 98 g/mol?

28 / 30

28. Which phenomenon (same molecular formula, different properties) Dalton’s theory could not explain?

29 / 30

29. Which set of compounds illustrates the Law of Reciprocal Proportions?

30 / 30

30. What is the mass of 5.6 L of oxygen gas at STP? (Molar mass = 32 g/mol)

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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. What is the molecular mass of carbon dioxide ()?

2 / 50

2. If the empirical formula of a compound is CH₂ and its molecular mass is 42, what is the molecular formula?

3 / 50

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

4 / 50

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

5 / 50

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

6 / 50

6. Which of the following processes demonstrates the combined role of chemistry and biology?

7 / 50

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

8 / 50

8. In , if 27 g of Al reacts with 73 g of HCl, which is limiting?

9 / 50

9. Calculate the percentage of calcium in 20 g of CaCO₃.

10 / 50

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

11 / 50

11. Which statement correctly describes molecular composition?

12 / 50

12. Which of the following laws is directly supported by the Law of Reciprocal Proportions?

13 / 50

13. In a reaction, 5 g of calcium reacts with 2 g of oxygen to form calcium oxide. The mass of CaO produced will be:

14 / 50

14. Which discovery disproved Dalton’s postulate of indivisible atoms?

15 / 50

15. How many atoms are present in 2 moles of aluminium?

16 / 50

16. Two oxides of nitrogen contain 30 g of nitrogen each. In one, oxygen is 34.3 g, and in the other, oxygen is 68.6 g. The ratio of masses of oxygen combining with nitrogen is:

17 / 50

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

18 / 50

18. Which of the following is a natural antioxidant found in green tea?

19 / 50

19. Which of the following correctly expresses the relation between moles and mass?

20 / 50

20. Which pair of gases would contain the same number of molecules at STP if taken in equal volumes?

21 / 50

21. In the reaction , 160 g Fe₂O₃ reacts with 84 g CO. Which is the limiting reagent?

22 / 50

22. If 0.5 moles of NaOH are present, what is the mass of NaOH? (Molar mass = 40 g/mol)

23 / 50

23. Which step is not necessary to determine an empirical formula experimentally?

24 / 50

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

25 / 50

25. How many grams of oxygen are present in 10 g of water ()?

26 / 50

26. Which modern concept can be seen as a direct extension of the Law of Reciprocal Proportions?

27 / 50

27. Why is it necessary to know the molecular mass when determining the molecular formula?

28 / 50

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

29 / 50

29. Which is a polyatomic elemental molecule?

30 / 50

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

31 / 50

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

32 / 50

32. Why do molecules of noble gases (He, Ne, Ar) exist as single atoms?

33 / 50

33. The law of conservation of mass was first proposed by:

34 / 50

34. What is meant by average atomic mass of an element?

35 / 50

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

36 / 50

36. Which of the following is the correct difference between atoms and molecules?

37 / 50

37. Which of the following statements is true about empirical formulas?

38 / 50

38. Which of the following pairs of compounds does not follow the Law of Multiple Proportions?

39 / 50

39. Which statement about atoms in chemical reactions is correct?

40 / 50

40. How many liters of CO₂ at STP are produced by complete combustion of 1 mole of CH₄? Reaction:

41 / 50

41. Which chemical process is the basis of the cement industry?

42 / 50

42. Which formula is correct for calculating average atomic mass?

43 / 50

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

44 / 50

44. The average atomic mass of lithium is 6.94 u. Which isotopes contribute to this value?

45 / 50

45. Who is credited with proposing the Law of Conservation of Mass?

46 / 50

46. In the combustion of methane, , if 16 g CH₄ and 64 g O₂ are used, the limiting reagent is:

47 / 50

47. The molar mass of sodium hydroxide (NaOH) is:

48 / 50

48. Which of the following statements is false?

49 / 50

49. How many molecules are there in 44 g of carbon dioxide (CO₂)?

50 / 50

50. What is the mass of calcium present in 50 g of calcium carbonate ()?

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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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  • Safety: This test is 100% free, and there are no hidden charges.

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