Exam-Style Online Test | Class 11 Chemistry: Basic Concepts

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. In determining empirical formula, why is the assumption of 100 g sample useful?

2 / 30

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

3 / 30

3. 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:

4 / 30

4. How many liters of hydrogen gas at STP are produced when 2 g of hydrogen is taken? (Molar mass H₂ = 2 g/mol)

5 / 30

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

6 / 30

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

7 / 30

7. Which statement about atomic mass unit is correct?

8 / 30

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

9 / 30

9. What is the atomicity of glucose ?

10 / 30

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

11 / 30

11. If the empirical formula mass and molecular mass are equal, what does it imply?

12 / 30

12. Which of the following compounds has a molecular mass of 18 u?

13 / 30

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

14 / 30

14. How many carbon atoms are in 1 mole of glucose ()?

15 / 30

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

16 / 30

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

17 / 30

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

18 / 30

18. Why is the empirical formula important in chemistry?

19 / 30

19. Which of the following is monoatomic at STP?

20 / 30

20. What is the empirical formula of acetic acid ()?

21 / 30

21. 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”?

22 / 30

22. What is meant by the molecular formula of a compound?

23 / 30

23. Which isotope is used as the standard reference for defining the atomic mass unit?

24 / 30

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

25 / 30

25. Who proposed Avogadro’s Hypothesis?

26 / 30

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

27 / 30

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

28 / 30

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

29 / 30

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

30 / 30

30. The SI unit of molar mass is:

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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. Where are protons and neutrons located in an atom?

2 / 50

2. What is meant by the empirical formula of a compound?

3 / 50

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

4 / 50

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

5 / 50

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

6 / 50

6. Which element exists as a polyatomic molecule under normal conditions?

7 / 50

7. Which statement is correct about monoatomic molecules?

8 / 50

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

9 / 50

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

10 / 50

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

11 / 50

11. Which equation illustrates a molecular chemical reaction?

12 / 50

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

13 / 50

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

14 / 50

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

15 / 50

15. 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:

16 / 50

16. Who proposed the Law of Definite Proportions?

17 / 50

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

18 / 50

18. Which of the following molecules is diatomic?

19 / 50

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

20 / 50

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

21 / 50

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

22 / 50

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

23 / 50

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

24 / 50

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

25 / 50

25. Which of the following chemicals is widely used in the fertilizer industry to enhance nitrogen content in soil?

26 / 50

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

27 / 50

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

28 / 50

28. How many molecules are present in 22 g of CO₂? (Molar mass = 44 g/mol)

29 / 50

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

30 / 50

30. Avogadro’s Hypothesis states that:

31 / 50

31. Why are atoms considered neutral?

32 / 50

32. Calculate the percentage of oxygen in water ().

33 / 50

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

34 / 50

34. Which formula relation is mathematically correct?

35 / 50

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

36 / 50

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

37 / 50

37. What is the atomicity of glucose ?

38 / 50

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

39 / 50

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

40 / 50

40. Which of the following correctly explains why mass is conserved in chemical reactions?

41 / 50

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

42 / 50

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

43 / 50

43. Which data is essential to calculate an empirical formula?

44 / 50

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

45 / 50

45. Which experiment supported Dalton’s idea that atoms combine in whole-number ratios?

46 / 50

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

47 / 50

47. Why is the Law of Conservation of Mass fundamental to balancing chemical equations?

48 / 50

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

49 / 50

49. In , what is the percentage of calcium?

50 / 50

50. Which of the following equations links mole, mass, and molar mass?

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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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