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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.

Get new questions on each attempt

  • Total Questions: 30
  • Time Allotted: 45 minutes
  • Passing Score: 50%
  • Randomization: Yes
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

Good luck! 👍

1 / 30

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

2 / 30

2. A sample of ammonia gas occupies 44.8 L at STP. How many molecules are present?

3 / 30

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

4 / 30

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

5 / 30

5. In a sample of water, the ratio of hydrogen to oxygen atoms is always:

6 / 30

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

7 / 30

7. Which of the following is the first postulate of Dalton’s Atomic Theory?

8 / 30

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

9 / 30

9. What is meant by the molar volume of a gas at STP?

10 / 30

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

11 / 30

11. Which law of chemical combination is directly explained by Dalton’s Atomic Theory?

12 / 30

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

13 / 30

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

14 / 30

14. According to Dalton’s postulates, atoms of a given element are:

15 / 30

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

16 / 30

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

17 / 30

17. The formula for percentage yield is:

18 / 30

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

19 / 30

19. Which branch of science deals with the study of composition, structure, and properties of matter?

20 / 30

20. Which experiment supported Avogadro’s Hypothesis?

21 / 30

21. Which of the following correctly links Avogadro’s number and molar mass?

22 / 30

22. 1 mole of water contains how many hydrogen atoms?

23 / 30

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

24 / 30

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

25 / 30

25. Which polymer is commonly used for making plastic bottles?

26 / 30

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

27 / 30

27. Which of the following is a polyatomic molecule?

28 / 30

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

29 / 30

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

30 / 30

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

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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 stoichiometric coefficient of CO₂ in the equation ?

2 / 50

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

3 / 50

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

4 / 50

4. Find the percentage of carbon in carbon dioxide ().

5 / 50

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

6 / 50

6. 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:

7 / 50

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

8 / 50

8. What is the percentage composition of Ca in CaCO₃?

9 / 50

9. Which statement about halogens is correct regarding atomicity at standard conditions?

10 / 50

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

11 / 50

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

12 / 50

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

13 / 50

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

14 / 50

14. Which branch of science deals with the study of composition, structure, and properties of matter?

15 / 50

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

16 / 50

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

17 / 50

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

18 / 50

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

19 / 50

19. Who proposed Avogadro’s Hypothesis?

20 / 50

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

21 / 50

21. The molecular mass of (ethane) is:

22 / 50

22. Why was Avogadro’s Hypothesis initially rejected?

23 / 50

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

24 / 50

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

25 / 50

25. Which of the following elements has an average atomic mass close to a whole number because it has only one stable isotope?

26 / 50

26. Which of the following fuels is considered the cleanest source of energy?

27 / 50

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

28 / 50

28. Which of the following is an incorrect pair of empirical and molecular formula?

29 / 50

29. In carbon dioxide (CO₂), the mass ratio of carbon to oxygen is:

30 / 50

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

31 / 50

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

32 / 50

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

33 / 50

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

34 / 50

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

35 / 50

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

36 / 50

36. Which experimental evidence supports Dalton’s Law of Multiple Proportions?

37 / 50

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

38 / 50

38. Which of the following is an industrial use of sulphuric acid, often called the “king of chemicals”?

39 / 50

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

40 / 50

40. Which of the following particles has the smallest mass in atomic mass units?

41 / 50

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

42 / 50

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

43 / 50

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

44 / 50

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

45 / 50

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

46 / 50

46. Which compound has 53.3% oxygen by mass?

47 / 50

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

48 / 50

48. What is meant by formula mass?

49 / 50

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

50 / 50

50. Which of the following is a diatomic molecule?

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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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