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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. What is the molar mass of nitrogen gas ()?

2 / 30

2. Why is percentage composition important in chemistry?

3 / 30

3. 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:

4 / 30

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

5 / 30

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

6 / 30

6. What is the atomicity of ammonium nitrate, ?

7 / 30

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

8 / 30

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

9 / 30

9. What is the formula mass of sodium chloride ()?

10 / 30

10. Which statement about metals in the solid state and atomicity is most accurate?

11 / 30

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

12 / 30

12. What is the atomicity of calcium hydroxide, ?

13 / 30

13. How many liters of oxygen gas are present at STP in 0.5 mole?

14 / 30

14. Which of the following is a triatomic molecule?

15 / 30

15. In 36 g of water, how much hydrogen is present?

16 / 30

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

17 / 30

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

18 / 30

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

19 / 30

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

20 / 30

20. Which engineering material is designed using chemical knowledge of polymers?

21 / 30

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

22 / 30

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

23 / 30

23. The molar mass of calcium carbonate () is:

24 / 30

24. Which concept of physics is essential to understand spectroscopy in chemistry?

25 / 30

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

26 / 30

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

27 / 30

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

28 / 30

28. What is the value of 1 atomic mass unit (amu) in grams?

29 / 30

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

30 / 30

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

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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 particle is directly rearranged during molecular chemical reactions?

2 / 50

2. The Law of Gaseous Volumes applies only to:

3 / 50

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

4 / 50

4. What is the mass of water formed when 2 g of H₂ reacts with excess O₂? Reaction:

5 / 50

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

6 / 50

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

7 / 50

7. Which law states: “When two elements combine to form two or more compounds, the masses of one element combining with a fixed mass of the other are in the ratio of small whole numbers”?

8 / 50

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

9 / 50

9. Dalton’s Atomic Theory helped in the development of:

10 / 50

10. The Haber process for ammonia synthesis demonstrates chemistry’s role in which field?

11 / 50

11. What is the formula mass of calcium carbonate ()?

12 / 50

12. Which experiment did Lavoisier perform to establish the Law of Conservation of Mass?

13 / 50

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

14 / 50

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

15 / 50

15. The molecular mass of (ethane) is:

16 / 50

16. A sample of CO₂ obtained from coal combustion contains 27.3% carbon and 72.7% oxygen. Another sample of CO₂ from fermentation contains 27.3% carbon and 72.7% oxygen. This confirms:

17 / 50

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

18 / 50

18. How many molecules of CO₂ are present in 22.4 L of CO₂ at STP?

19 / 50

19. Which condition is necessary to apply Gay-Lussac’s Law of Gaseous Volumes correctly?

20 / 50

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

21 / 50

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

22 / 50

22. What is the molar mass of glucose ()?

23 / 50

23. Which of the following compounds has different empirical and molecular formulas?

24 / 50

24. The role of chemistry in engineering is most clearly seen in which example?

25 / 50

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

26 / 50

26. The Law of Definite Proportions states that:

27 / 50

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

28 / 50

28. Which technology relies on the semiconductor properties of silicon, discovered through chemical purification?

29 / 50

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

30 / 50

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

31 / 50

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

32 / 50

32. 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:

33 / 50

33. Who proposed the Law of Multiple Proportions?

34 / 50

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

35 / 50

35. Which of the following is not a limitation of Dalton’s theory (i.e., it is actually a strength/merit)?

36 / 50

36. Which of the following compounds has a formula mass of 142 u?

37 / 50

37. In the reaction , if 1 mole C₂H₆ is burned with 2 moles O₂, which is limiting?

38 / 50

38. Which engineering material is designed using chemical knowledge of polymers?

39 / 50

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

40 / 50

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

41 / 50

41. Which equation best illustrates a chemical reaction at the atomic level?

42 / 50

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

43 / 50

43. Which of the following compounds has atomicity 7?

44 / 50

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

45 / 50

45. In , the percentage of chlorine is:

46 / 50

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

47 / 50

47. Which chemical compound is responsible for the pungent smell of onions?

48 / 50

48. Which of the following is an extensive property?

49 / 50

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

50 / 50

50. Which concept of physics is essential to understand spectroscopy in chemistry?

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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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  • Best experience: Use a stable internet connection and the latest browser for the best performance.
  • 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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