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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 of the following represents a molecule and not a single atom?

2 / 30

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

3 / 30

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

4 / 30

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

5 / 30

5. Which branch of physics directly supports chemistry in explaining atomic orbitals?

6 / 30

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

7 / 30

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

8 / 30

8. Which of the following is not an importance of chemistry in everyday life?

9 / 30

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

10 / 30

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

11 / 30

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

12 / 30

12. Dalton’s postulate that atoms are indestructible fails in which processes?

13 / 30

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

14 / 30

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

15 / 30

15. Which postulate explains the Law of Multiple Proportions?

16 / 30

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

17 / 30

17. Which of the following is an extensive property?

18 / 30

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

19 / 30

19. Which of the following statements is false?

20 / 30

20. Which of the following best illustrates the Law of Multiple Proportions?

21 / 30

21. 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:

22 / 30

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

23 / 30

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

24 / 30

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

25 / 30

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

26 / 30

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

27 / 30

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

28 / 30

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

29 / 30

29. Which information cannot be obtained directly from the molecular formula?

30 / 30

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

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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 formula mass of potassium sulfate ()?

2 / 50

2. Which of the following molecules is diatomic?

3 / 50

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

4 / 50

4. Which reaction shows molecular decomposition?

5 / 50

5. 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:

6 / 50

6. What is the definition of a mole in chemistry?

7 / 50

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

8 / 50

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

9 / 50

9. In the reaction , what mass of AlCl₃ is formed from 54 g of Al (assuming 100% yield)?

10 / 50

10. The empirical formula of glucose (C₆H₁₂O₆) is:

11 / 50

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

12 / 50

12. Which of the following shows chemistry’s importance in modern agriculture?

13 / 50

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

14 / 50

14. Which of the following is a triatomic molecule?

15 / 50

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

16 / 50

16. What is meant by formula mass?

17 / 50

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

18 / 50

18. Why is molecular formula considered more informative than empirical formula?

19 / 50

19. Which statement correctly describes molecular composition?

20 / 50

20. In the reaction of carbon monoxide and oxygen: , the volume ratio of CO : O₂ : CO₂ is:

21 / 50

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

22 / 50

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

23 / 50

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

24 / 50

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

25 / 50

25. Who proposed Avogadro’s Hypothesis?

26 / 50

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

27 / 50

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

28 / 50

28. In the reaction , the theoretical yield is 36 g H₂O. If the actual yield is 30 g, what is the percentage yield?

29 / 50

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

30 / 50

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

31 / 50

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

32 / 50

32. 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:

33 / 50

33. Who proposed the Law of Definite Proportions?

34 / 50

34. The study of enzymes acting as catalysts in biochemical reactions is an overlap of:

35 / 50

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

36 / 50

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

37 / 50

37. Which formula is used to calculate molecular mass?

38 / 50

38. In the reaction , how many moles of water are formed when 4 moles of hydrogen react with excess oxygen?

39 / 50

39. 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:

40 / 50

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

41 / 50

41. Magnesium has three isotopes: Mg-24 (79%), Mg-25 (10%), and Mg-26 (11%). What is the average atomic mass?

42 / 50

42. Find the oxygen mass in 88 g of CO₂.

43 / 50

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

44 / 50

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

45 / 50

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

46 / 50

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

47 / 50

47. Which calculation correctly shows the number of oxygen atoms in 0.5 mole of O₂?

48 / 50

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

49 / 50

49. 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:

50 / 50

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

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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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