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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. Which statement is true about empirical and molecular formulas?

2 / 30

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

3 / 30

3. Why was the Law of Reciprocal Proportions important historically?

4 / 30

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

5 / 30

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

6 / 30

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

7 / 30

7. Which of the following samples contains the largest number of molecules?

8 / 30

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

9 / 30

9. Dalton’s fixed-composition view of compounds is limited because some solids are non-stoichiometric. Which is a classic example?

10 / 30

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

11 / 30

11. Why is the Law of Multiple Proportions important in chemistry?

12 / 30

12. Which experiment supported Avogadro’s Hypothesis?

13 / 30

13. In the steel industry, chemistry is crucial for:

14 / 30

14. Which of the following is used as an antacid to reduce acidity in the stomach?

15 / 30

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

16 / 30

16. Which of the following statements is false?

17 / 30

17. How many hydrogen atoms are in 1 mole of methane ()?

18 / 30

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

19 / 30

19. The molecular formula of hydrogen peroxide is H₂O₂. What is its empirical formula?

20 / 30

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

21 / 30

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

22 / 30

22. Which statement best describes the Law of Multiple Proportions?

23 / 30

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

24 / 30

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

25 / 30

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

26 / 30

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

27 / 30

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

28 / 30

28. Which of the following correctly represents the atomic composition of oxygen-16?

29 / 30

29. If a compound has empirical formula CH and molar mass 78 g/mol, what is the molecular formula?

30 / 30

30. Which set contains only triatomic molecules?

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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. Which chemical is commonly used as an artificial sweetener in food products?

2 / 50

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

3 / 50

3. Which of the following best defines a molecule?

4 / 50

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

5 / 50

5. Which branch of chemistry is most relevant for developing renewable energy technologies like solar cells?

6 / 50

6. In NO and NO₂, 14 g of nitrogen combines with 16 g and 32 g of oxygen, respectively. The ratio of masses of oxygen is:

7 / 50

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

8 / 50

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

9 / 50

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

10 / 50

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

11 / 50

11. Which chemical is responsible for the preservation of food in pickles?

12 / 50

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

13 / 50

13. Which of the following reactions best demonstrates the Law of Conservation of Mass?

14 / 50

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

15 / 50

15. Avogadro’s number is numerically equal to:

16 / 50

16. Which of the following best represents Dalton’s view of chemical reactions?

17 / 50

17. Which of the following is a polyatomic molecule?

18 / 50

18. Which of the following compounds has atomicity 7?

19 / 50

19. In the combustion reaction , what is the coefficient of CO₂?

20 / 50

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

21 / 50

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

22 / 50

22. In H₂O, 2 g of hydrogen combines with 16 g of oxygen. In H₂S, 2 g of hydrogen combines with 32 g of sulphur. According to Richter’s law, the ratio of masses of oxygen and sulphur that combine with each other should be:

23 / 50

23. Where are protons and neutrons located in an atom?

24 / 50

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

25 / 50

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

26 / 50

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

27 / 50

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

28 / 50

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

29 / 50

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

30 / 50

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

31 / 50

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

32 / 50

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

33 / 50

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

34 / 50

34. Why are mole ratios sometimes multiplied by 2, 3, or 4 during empirical formula calculation?

35 / 50

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

36 / 50

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

37 / 50

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

38 / 50

38. What is the molecular mass of ?

39 / 50

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

40 / 50

40. The empirical formula of acetic acid is CH₂O. If its molar mass is 60 g/mol, what is its molecular formula?

41 / 50

41. What is the stoichiometric coefficient of CO₂ in the equation ?

42 / 50

42. The concept of alloys like brass and bronze shows the relation of chemistry with:

43 / 50

43. Who proposed the Law of Multiple Proportions?

44 / 50

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

45 / 50

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

46 / 50

46. Which reaction verifies Gay-Lussac’s Law?

47 / 50

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

48 / 50

48. The number is known as:

49 / 50

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

50 / 50

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

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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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