Exam-Style Online Test | Class 11 Chemistry: Basic Concepts
GK Aim: A Treasure of MCQs

Class 11 Chemistry — Chapter 1: Some Basic Concepts of Chemistry Online Test

Start Your Test by Choosing a Paper

0%

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?

Please provide information to view your result.

Your score is

Share your achievement!

LinkedIn Facebook Twitter
0%

Please provide your feedback.

Thank you for your valuable feedback.

0%

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 statement best summarizes Gay-Lussac’s Law of Gaseous Volumes?

2 / 30

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

3 / 30

3. Which is a polyatomic elemental molecule?

4 / 30

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

5 / 30

5. Which of the following is a triatomic molecule?

6 / 30

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

7 / 30

7. Which of the following is a polyatomic molecule?

8 / 30

8. 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:

9 / 30

9. Which of the following statements is false?

10 / 30

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

11 / 30

11. Which formula is derived from Avogadro’s Hypothesis?

12 / 30

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

13 / 30

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

14 / 30

14. Which experimental evidence supported Proust’s Law?

15 / 30

15. Which technology relies on the semiconductor properties of silicon, discovered through chemical purification?

16 / 30

16. Which experiment supported Avogadro’s Hypothesis?

17 / 30

17. Which discovery proved Dalton wrong about atoms of an element being identical?

18 / 30

18. Which of the following is monoatomic at STP?

19 / 30

19. Which scientist first introduced the modern concept of the atom?

20 / 30

20. Which of the following is the correct difference between atoms and molecules?

21 / 30

21. In the reaction , how many grams of AlCl₃ are produced from 54 g of Al?

22 / 30

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

23 / 30

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

24 / 30

24. What is the atomicity of glucose ?

25 / 30

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

26 / 30

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

27 / 30

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

28 / 30

28. Which compound has 53.3% oxygen by mass?

29 / 30

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

30 / 30

30. Why are noble gases (e.g., Ar, Ne) classified as atoms rather than molecules?

Please provide information to view your result.

Your score is

Share your achievement!

LinkedIn Facebook Twitter
0%

Please provide your feedback.

Thank you for your valuable feedback.

0%

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!

Earn a certificate upon passing

Get new questions with every attempt

  • 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 chemical is used in the agriculture industry as a pesticide?

2 / 50

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

3 / 50

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

4 / 50

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

5 / 50

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

6 / 50

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

7 / 50

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

8 / 50

8. Which equation illustrates a molecular chemical reaction?

9 / 50

9. Who proposed the Law of Gaseous Volumes?

10 / 50

10. What is the atomicity of calcium hydroxide, ?

11 / 50

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

12 / 50

12. Which statement best summarizes Gay-Lussac’s Law of Gaseous Volumes?

13 / 50

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

14 / 50

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

15 / 50

15. Which of the following gases is monoatomic in nature?

16 / 50

16. The Haber process, an industrial application of equilibrium chemistry, is used to manufacture:

17 / 50

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

18 / 50

18. Which formula is derived from Avogadro’s Hypothesis?

19 / 50

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

20 / 50

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

21 / 50

21. What is the atomicity of sulphur in its most stable molecular form?

22 / 50

22. Which of the following correctly represents the atomicity of ozone?

23 / 50

23. Which of the following provides direct evidence for Avogadro’s Hypothesis?

24 / 50

24. Which of the following compounds does not obey the Law of Definite Proportions strictly?

25 / 50

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

26 / 50

26. What is meant by molar mass of a substance?

27 / 50

27. Which formula is used to calculate molecular mass?

28 / 50

28. Which of the following is a heteronuclear molecule?

29 / 50

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

30 / 50

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

31 / 50

31. 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:

32 / 50

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

33 / 50

33. Why is molecular mass important in chemistry?

34 / 50

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

35 / 50

35. How many grams of NaCl are formed when 5.85 g Na reacts with excess Cl₂? Reaction:

36 / 50

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

37 / 50

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

38 / 50

38. Dalton’s Atomic Theory helped in the development of:

39 / 50

39. For the reaction , what is the stoichiometric coefficient of ammonia?

40 / 50

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

41 / 50

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

42 / 50

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

43 / 50

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

44 / 50

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

45 / 50

45. Which particle is responsible for the chemical behavior of an atom?

46 / 50

46. The molecular mass of (ethane) is:

47 / 50

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

48 / 50

48. The mass of a hydrogen atom is approximately:

49 / 50

49. Which of the following statements is true about empirical formulas?

50 / 50

50. Which discovery proved Dalton wrong about atoms of an element being identical?

Please provide accurate information so we can send your Achievement Certificate by mail.

Your score is

Share your achievement!

LinkedIn Facebook Twitter
0%

Please provide your feedback.

Thank you for your valuable feedback.

Practice Some Basic Concepts of Chemistry MCQs
Download Class 11 Chemistry MCQ Study Bundle

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)

  • Do not refresh or close the tab during the test, as it may disrupt your session.
  • Best experience: Use a stable internet connection and the latest browser for the best performance.
  • Allow cookies / local storage to save your progress and results.
  • Safety: This test is 100% free, and there are no hidden charges.

FAQs on Some Basic Concepts of Chemistry Online Test ▼

Subscribe
Notify of
guest
0 Comments
Inline Feedbacks
View all comments

Related MCQs

Scroll to Top