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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. Which example shows a variable composition compound that challenges Dalton’s fixed whole-number ratios?

2 / 30

2. What is meant by actual yield of a reaction?

3 / 30

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

4 / 30

4. Which statement about atoms in chemical reactions is correct?

5 / 30

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

6 / 30

6. Which experiment supported Avogadro’s Hypothesis?

7 / 30

7. Which is the correct molecular mass of ammonia ()?

8 / 30

8. What is the molecular mass of carbon dioxide ()?

9 / 30

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

10 / 30

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

11 / 30

11. In the reaction , if 5 moles of H₂ and 2 moles of O₂ are mixed, which is the limiting reagent?

12 / 30

12. Sulfur vapour at very high temperature contains . The atomicity of is:

13 / 30

13. Who proposed the Law of Reciprocal Proportions?

14 / 30

14. What are the stoichiometric coefficients of reactants in the neutralization reaction ?

15 / 30

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

16 / 30

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

17 / 30

17. Which compound has 53.3% oxygen by mass?

18 / 30

18. In the balanced equation , what is the stoichiometric coefficient of oxygen?

19 / 30

19. The Solvay process is used in the chemical industry to produce:

20 / 30

20. 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:

21 / 30

21. What is the atomicity of calcium hydroxide, ?

22 / 30

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

23 / 30

23. What does the term atomicity refer to?

24 / 30

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

25 / 30

25. What is the relation between 1 mole of carbon-12 atoms and amu?

26 / 30

26. Which is the first requirement to determine molecular formula experimentally?

27 / 30

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

28 / 30

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

29 / 30

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

30 / 30

30. In the reaction , 160 g Fe₂O₃ reacts with 84 g CO. Which is the limiting reagent?

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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 meant by actual yield of a reaction?

2 / 50

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

3 / 50

3. In the reaction , if 5 moles of H₂ and 2 moles of O₂ are mixed, which is the limiting reagent?

4 / 50

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

5 / 50

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

6 / 50

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

7 / 50

7. Which merit of Dalton’s Atomic Theory connects directly with the development of the mole concept?

8 / 50

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

9 / 50

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

10 / 50

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

11 / 50

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

12 / 50

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

13 / 50

13. What is the stoichiometric coefficient of CO₂ in the equation ?

14 / 50

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

15 / 50

15. Which chemical process is the basis of the cement industry?

16 / 50

16. Which interdisciplinary area combines chemistry and physics for medical imaging technologies like MRI?

17 / 50

17. Dalton did not distinguish clearly between atoms and molecules (e.g., he treated elemental gases as monatomic). Which idea resolved this?

18 / 50

18. What is the percentage composition of nitrogen in ammonia ()?

19 / 50

19. Which merit of Dalton’s theory laid the foundation for modern chemistry?

20 / 50

20. Which of the following has the highest molecular mass?

21 / 50

21. Sulfur vapour at very high temperature contains . The atomicity of is:

22 / 50

22. When 2 volumes of hydrogen combine with 1 volume of oxygen, the product formed is:

23 / 50

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

24 / 50

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

25 / 50

25. Which postulate explains the Law of Conservation of Mass?

26 / 50

26. Why is molecular mass important in chemistry?

27 / 50

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

28 / 50

28. Which statement is true about formula mass?

29 / 50

29. Which merit of Dalton’s theory helped establish chemical formulae?

30 / 50

30. If 67.2 L of hydrogen gas is taken at STP, how many moles does it represent?

31 / 50

31. What is the atomicity of calcium hydroxide, ?

32 / 50

32. Which of the following is not a postulate of Dalton’s Atomic Theory?

33 / 50

33. Why is chemistry considered central among sciences?

34 / 50

34. Which compound is often cited as an example of the Law of Definite Proportions?

35 / 50

35. How many grams of NaOH are required to neutralize 49 g of H₂SO₄? Reaction:

36 / 50

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

37 / 50

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

38 / 50

38. Which reaction shows molecular decomposition?

39 / 50

39. Why are mole ratios sometimes multiplied by 2, 3, or 4 during empirical formula calculation?

40 / 50

40. Which experiment supported Avogadro’s Hypothesis?

41 / 50

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

42 / 50

42. The approximate mass of one proton is:

43 / 50

43. Which of the following explains why average atomic masses are often decimal numbers?

44 / 50

44. Which of the following compounds requires the use of formula mass rather than molecular mass?

45 / 50

45. If 0.5 moles of NaOH are present, what is the mass of NaOH? (Molar mass = 40 g/mol)

46 / 50

46. In the reaction: the ratio of volumes of hydrogen, chlorine, and hydrogen chloride is:

47 / 50

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

48 / 50

48. Which of the following compounds has atomicity 7?

49 / 50

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

50 / 50

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

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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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