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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. The number is known as:

2 / 30

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

3 / 30

3. Which of the following is equal to 1 mole of oxygen gas ()?

4 / 30

4. Why is Dalton’s Atomic Theory still important today despite its limitations?

5 / 30

5. How many liters of hydrogen gas at STP are produced when 2 g of hydrogen is taken? (Molar mass H₂ = 2 g/mol)

6 / 30

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

7 / 30

7. Which of the following best describes how Dalton’s theory supported the Law of Multiple Proportions?

8 / 30

8. Chlorine occurs in two isotopes: Cl-35 (75% abundance) and Cl-37 (25% abundance). What is the average atomic mass of chlorine?

9 / 30

9. Why is the empirical formula important in chemistry?

10 / 30

10. Why is chemistry considered central among sciences?

11 / 30

11. Which isotope is used as the standard reference for defining the atomic mass unit?

12 / 30

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

13 / 30

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

14 / 30

14. Which of the following is a diatomic molecule?

15 / 30

15. If 88 g of CO₂ are taken, how many moles are present? (Molar mass of CO₂ = 44 g/mol)

16 / 30

16. Which postulate explains the Law of Conservation of Mass?

17 / 30

17. If 67.2 L of hydrogen gas is taken at STP, how many moles does it represent?

18 / 30

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

19 / 30

19. Which chemical principle helps engineers design batteries for electric vehicles?

20 / 30

20. Which discovery first showed that atoms are divisible, contradicting Dalton’s “indivisible atom” postulate?

21 / 30

21. Why was Dalton’s Atomic Theory considered revolutionary at the time?

22 / 30

22. How many particles are present in 2 moles of sodium chloride (NaCl)?

23 / 30

23. Which of the following is an example where the molecular and empirical formula are the same?

24 / 30

24. Which discovery proved Dalton wrong about atoms of an element being identical?

25 / 30

25. In the equation , the coefficient of hydrogen gas is:

26 / 30

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

27 / 30

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

28 / 30

28. If the mole ratios are not whole numbers (e.g., 1 : 1.5 : 2), what should be done?

29 / 30

29. If the empirical formula of a compound is CH₂ and its molar mass is 28 g/mol, what is the molecular formula?

30 / 30

30. Which of the following statements is false?

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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. The Law of Gaseous Volumes applies only to:

2 / 50

2. Why is the average atomic mass of chlorine not exactly 36 u, even though it has Cl-35 and Cl-37 isotopes?

3 / 50

3. According to Dalton’s Atomic Theory, matter is composed of:

4 / 50

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

5 / 50

5. Which concept directly arises from Avogadro’s Hypothesis?

6 / 50

6. What does the term atomicity refer to?

7 / 50

7. Which fertilizer provides both nitrogen and phosphorus to crops?

8 / 50

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

9 / 50

9. For the reaction , what is the stoichiometric coefficient of ammonia?

10 / 50

10. How many grams of NaOH are required to neutralize 49 g of H₂SO₄? Reaction:

11 / 50

11. In the reaction , if 44 g of propane burns, how many liters of CO₂ at STP are produced?

12 / 50

12. Which of the following correctly represents 1 mole of oxygen gas?

13 / 50

13. Which compound has 53.3% oxygen by mass?

14 / 50

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

15 / 50

15. Why is the Law of Definite Proportions important in chemistry?

16 / 50

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

17 / 50

17. Why is the concept of a limiting reagent important in chemistry?

18 / 50

18. Why is percentage composition important in chemistry?

19 / 50

19. Which of the following is the correct SI unit of amount of substance?

20 / 50

20. Which is correct about molar volume of gases at STP?

21 / 50

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

22 / 50

22. What is meant by molar mass of a substance?

23 / 50

23. What is meant by theoretical yield of a chemical reaction?

24 / 50

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

25 / 50

25. Which of the following gases is monoatomic in nature?

26 / 50

26. What is the atomicity of ammonium nitrate, ?

27 / 50

27. Which of the following is not a postulate of Dalton’s Atomic Theory?

28 / 50

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

29 / 50

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

30 / 50

30. Which of the following is an example of an atom but not a molecule?

31 / 50

31. What is the percentage of carbon in carbon dioxide ()?

32 / 50

32. Which equation illustrates a molecular chemical reaction?

33 / 50

33. How many moles of oxygen gas are present in 44.8 L of O₂ at STP?

34 / 50

34. Who proposed the Law of Definite Proportions?

35 / 50

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

36 / 50

36. A sample of calcium carbonate (CaCO₃) has a mass of 100 g. What is the number of moles present?

37 / 50

37. On what standard is the modern atomic mass unit based?

38 / 50

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

39 / 50

39. The Haber process, an industrial application of equilibrium chemistry, is used to manufacture:

40 / 50

40. What is the main difference between an empirical formula and a molecular formula?

41 / 50

41. Which of the following correctly distinguishes molecular mass and formula mass?

42 / 50

42. The mass of one atom of oxygen-16 isotope is:

43 / 50

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

44 / 50

44. Why was Dalton’s Atomic Theory considered revolutionary at the time?

45 / 50

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

46 / 50

46. If 4 g of hydrogen reacts with 32 g of oxygen, which is the limiting reagent in ?

47 / 50

47. Which of the following correctly lists the three fundamental subatomic particles in an atom?

48 / 50

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

49 / 50

49. Which of the following correctly gives the percentage composition of oxygen in sulphur dioxide ()?

50 / 50

50. Which of the following statements is false?

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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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  • Allow cookies / local storage to save your progress and results.
  • Safety: This test is 100% free, and there are no hidden charges.

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