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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 statements is false?

2 / 30

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

3 / 30

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

4 / 30

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

5 / 30

5. Avogadro’s number is numerically equal to:

6 / 30

6. Which reaction shows molecular decomposition?

7 / 30

7. Which of the following processes demonstrates the combined role of chemistry and biology?

8 / 30

8. Which of the following is true about the mole concept?

9 / 30

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

10 / 30

10. Which of the following is an extensive property?

11 / 30

11. The molar mass of ammonia () is:

12 / 30

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

13 / 30

13. Which allotrope of oxygen has atomicity 3?

14 / 30

14. Which postulate of Dalton’s Atomic Theory helped in introducing the concept of molecular masses?

15 / 30

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

16 / 30

16. In CO and CO₂, 12 g of carbon combines with 16 g and 32 g of oxygen, respectively. The ratio of masses of oxygen combining with the same mass of carbon is:

17 / 30

17. The number is known as:

18 / 30

18. Which of the following is true about molecules but not about atoms?

19 / 30

19. Which of the following is a triatomic molecule?

20 / 30

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

21 / 30

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

22 / 30

22. Why is atomicity an important concept?

23 / 30

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

24 / 30

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

25 / 30

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

26 / 30

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

27 / 30

27. Which of the following statements from Dalton’s theory is still valid today?

28 / 30

28. 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:

29 / 30

29. Who proposed Avogadro’s Hypothesis?

30 / 30

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

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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 engineering material is designed using chemical knowledge of polymers?

2 / 50

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

3 / 50

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

4 / 50

4. Why is the atomic mass unit more convenient than grams in chemistry?

5 / 50

5. Which element pair and common element verify the Law of Reciprocal Proportions?

6 / 50

6. Which of the following is monoatomic at STP?

7 / 50

7. Why is molar mass important in stoichiometric calculations?

8 / 50

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

9 / 50

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

10 / 50

10. What is the mass of calcium present in 50 g of calcium carbonate ()?

11 / 50

11. Gay-Lussac’s law of gaseous volumes was one of the foundations for which later concept?

12 / 50

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

13 / 50

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

14 / 50

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

15 / 50

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

16 / 50

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

17 / 50

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

18 / 50

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

19 / 50

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

20 / 50

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

21 / 50

21. Which of the following statements from Dalton’s theory is still valid today?

22 / 50

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

23 / 50

23. In the balanced combustion reaction of methane: , what is the coefficient of water?

24 / 50

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

25 / 50

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

26 / 50

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

27 / 50

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

28 / 50

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

29 / 50

29. The Law of Reciprocal Proportions states that:

30 / 50

30. The number of oxygen atoms in 18 g of water is:

31 / 50

31. Which of the following shows the correct relation between mole and volume of a gas at STP?

32 / 50

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

33 / 50

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

34 / 50

34. The SI unit of molar mass is:

35 / 50

35. In the equation , the coefficients of products are:

36 / 50

36. The molar volume of a gas at STP is:

37 / 50

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

38 / 50

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

39 / 50

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

40 / 50

40. What is meant by formula mass?

41 / 50

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

42 / 50

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

43 / 50

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

44 / 50

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

45 / 50

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

46 / 50

46. Which of the following correctly compares molecular formula vs empirical formula?

47 / 50

47. The molar mass of ammonia () is:

48 / 50

48. Which merit of Dalton’s theory helped explain the Law of Definite Proportions?

49 / 50

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

50 / 50

50. 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:

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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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