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

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. Who proposed the Law of Reciprocal Proportions?

2 / 30

2. In the reaction , if 10 moles of N₂ and 15 moles of H₂ are available, what is the limiting reagent?

3 / 30

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

4 / 30

4. Determine the atomicity of (ammonium sulfate).

5 / 30

5. How many moles of oxygen are required to completely combust 2 moles of ethane ()? Reaction:

6 / 30

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

7 / 30

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

8 / 30

8. Who is credited with proposing the first modern atomic theory?

9 / 30

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

10 / 30

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

11 / 30

11. The study of pollutants in rivers and their effect on aquatic life shows the connection of chemistry with:

12 / 30

12. Which of the following is true about the relation between mole, mass, and volume?

13 / 30

13. Which reaction shows molecular decomposition?

14 / 30

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

15 / 30

15. Which fertilizer provides both nitrogen and phosphorus to crops?

16 / 30

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

17 / 30

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

18 / 30

18. Why is molecular mass important in chemistry?

19 / 30

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

20 / 30

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

21 / 30

21. Which of the following is monoatomic at STP?

22 / 30

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

23 / 30

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

24 / 30

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

25 / 30

25. Which compound has 53.3% oxygen by mass?

26 / 30

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

27 / 30

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

28 / 30

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

29 / 30

29. Who is credited with proposing the Law of Conservation of Mass?

30 / 30

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

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

2 / 50

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

3 / 50

3. Why is chemistry considered central among sciences?

4 / 50

4. The empirical formula of acetic acid is CH₂O. If its molar mass is 60 g/mol, what is its molecular formula?

5 / 50

5. In a sample of water, the ratio of hydrogen to oxygen atoms is always:

6 / 50

6. In an experiment, 10 g of a hydrocarbon is completely burnt in oxygen to form 30 g of CO₂ and 9 g of H₂O. What is the mass of oxygen consumed?

7 / 50

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

8 / 50

8. If the mole ratios are not whole numbers (e.g., 1 : 1.5 : 2), what should be done?

9 / 50

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

10 / 50

10. According to Dalton’s Atomic Theory, matter is composed of:

11 / 50

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

12 / 50

12. Which of the following combinations does NOT illustrate the Law of Reciprocal Proportions?

13 / 50

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

14 / 50

14. Which statement is correct about monoatomic molecules?

15 / 50

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

16 / 50

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

17 / 50

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

18 / 50

18. 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:

19 / 50

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

20 / 50

20. Which of the following is not true about molar volume of gases?

21 / 50

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

22 / 50

22. Which of the following compounds has atomicity 7?

23 / 50

23. Who proposed the Law of Gaseous Volumes?

24 / 50

24. Which statement about atomic mass unit is correct?

25 / 50

25. Which equation best illustrates a chemical reaction at the atomic level?

26 / 50

26. Which of the following correctly links Avogadro’s number and molar mass?

27 / 50

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

28 / 50

28. How many atoms are present in 2 moles of aluminium?

29 / 50

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

30 / 50

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

31 / 50

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

32 / 50

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

33 / 50

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

34 / 50

34. Which statement is true about formula mass?

35 / 50

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

36 / 50

36. The average atomic mass of lithium is 6.94 u. Which isotopes contribute to this value?

37 / 50

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

38 / 50

38. Which of the following is an extensive property?

39 / 50

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

40 / 50

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

41 / 50

41. What is meant by formula mass?

42 / 50

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

43 / 50

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

44 / 50

44. Who is credited with proposing the Law of Conservation of Mass?

45 / 50

45. Dalton’s postulates emphasized that compounds are formed by:

46 / 50

46. 1 mole of water contains how many hydrogen atoms?

47 / 50

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

48 / 50

48. What mass of carbon dioxide is present in 2 moles?

49 / 50

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

50 / 50

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

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