: Priti Singhal
: NEET National Eligibility Cum Entrance Test Chemistry Class 11 + 12 Volume I + Volume II
: Poorav Publications
: 9789348762368
: 1
: CHF 6.60
:
: Chemie
: English
: 296
: DRM
: PC/MAC/eReader/Tablet
: ePUB

Preparing for the NEET National Eligibility Cum Entrance Test Chemistry Class 11 + 12 Volume I + Volume II is a significant milestone for students aspiring to join the medical and dental fields. This book is designed to be a comprehensive guide for NEET preparation, addressing all aspects of the syllabus with clear concepts, practice materials, and exam strategies. It aims to help students understand subjects thoroughly while developing the skills to solve problems efficiently under time pressure.
The content in this book has been meticulously aligned with the latest NEET syllabus and trends, reflecting insights from previous years' papers. We have focused on high-yield topics and included chapter summaries, topic-wise MCQs, and mock tests to provide a structured approach to learning. Whether it's mastering Biology, tackling numerical in Physics, or understanding the complexities of Organic Chemistry, this book offers step-by-step solutions to help students at every stage of their preparation.
One of the unique features of this book is the integration of past year questions within chapters to show how theoretical concepts are applied in actual NEET exams. Full-length mock tests have also been provided to simulate the exact exam environment, building speed and confidence. For students struggling with time management, we offer strategies to plan daily schedules effectively and balance study and relaxation to avoid burnout.
Preparing for NEET can be challenging, and staying motivated throughout the journey is crucial. To inspire students, we've included tips and success stories from previous NEET toppers, demonstrating that success is within reach with consistent effort and the right strategies.
We recommend that students identify their strengths and weaknesses early on, focus on regular practice, and use mock tests to monitor progress. NEET is a demanding exam, but every student can succeed with dedication, proper guidance, and efficient planning.
We sincerely thank the educators, students, and contributors who helped make this book possible. Their insights and feedback have been invaluable in refining the content. We hope this book becomes a trusted companion on your NEET journey and helps you achieve your dream of joining a medical college.
I wish you all the best for your preparation and success in the NEET exam!

CHAPTER 1


Some Basic Concepts of Chemistry

 

1. Which law states that a chemical reaction can neither create nor destroy mass?

a) Law of Definite Proportions

b) Law of Conservation of Mass✔️

c) Law of Multiple Proportions

d) Avogadro’s Law

 

2. Who gave the Law of Multiple Proportions?

a) John Dalton✔️

b) Joseph Proust

c) Antoine Lavoisier

d) Robert Boyle

 

3. Which law states that a chemical compound always contains the same elements in the same proportion by mass?

a) Law of Definite Proportions✔️

b) Law of Conservation of Mass

c) Law of Multiple Proportions

d) Dalton’s Law

 

4. Dalton’s atomic theory explains:

a) Nuclear reactions

b) Law of Definite Proportions✔️

c) Radioactivity

d) Behavior of gases

 

5. The molecular mass of oxygen (O₂) is:

a) 16 amu

b) 32 amu✔️

c) 18 amu

d) 44 amu

 

6. How many molecules are present in 1 mole of a substance?

a) 3.011 × 10²³

b) 6.022 × 10²³✔️

c) 1.602 × 10⁻¹⁹

d) 9.8 × 10⁸

 

7. The molar mass of water (H₂O) is:

a) 16 g/mol

b) 18 g/mol✔️

c) 32 g/mol

d) 44 g/mol

 

8. What is the empirical formula of glucose (C₆H₁₂O₆)?

a) CH₂O✔️

b) C₂H₄O₂

c) C₆H₆

d) CH₄

 

9. In which compound is the mass ratio of hydrogen to oxygen 1:8?

a) H₂O✔️

b) H₂O₂

c) CO₂

d) NaOH

 

10. What is the percentage of carbon in methane (CH₄)? (C = 12, H = 1)

a) 75%✔️

b) 50%

c) 25%

d) 12.5%

 

11. What is the mass of 1 mole of nitrogen gas (N₂)?

a) 14 g

b) 28 g✔️

c) 32 g

d) 44 g

 

12. How many grams are present in 0.5 moles of CO₂? (Molar mass of CO₂ = 44 g/mol)

a) 11 g

b) 22 g✔️

c) 44 g

d) 88 g

 

13. The ratio of atoms in the empirical formula of a compound with molecular formula C₂H₄ is:

a) 1:1

b) 1:2✔️

c) 2:1

d) 3:1

 

14. Which gas has a molar mass of 2 g/mol?

a) Helium

b) Hydrogen✔️

c) Oxygen

d) Nitrogen

 

15. How many atoms are in 0.5 moles of oxygen gas (O₂)?

a) 3.011 × 10²³✔️

b) 6.022 × 10²³

c) 1.204 × 10²⁴

d) 9.033 × 10²³

 

16. Which of the following compounds has the highest percentage of oxygen?

a) H₂O✔️

b) CO₂

c) CH₄

d) NH₃

 

17. What is the percentage composition of hydrogen in water? (H₂O)

a) 11.1%✔️

b) 18.0%

c) 8.0%

d) 50%

 

18. What is the molecular formula of a compound with empirical formula CH₂ and molar mass 42 g/mol?

a) C₂H₄

b) C₃H₆✔️

c) C₄H₈

d) CH₄

 

19. How many moles of hydrogen are present in 1 mole of H₂O?

a) 1

b) 2✔️

c) 0.5

d) 3

 

20. What is the stoichiometric coefficient of oxygen in the equation: 2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O?

a) 8

b) 10

c) 13✔️

d) 2

 

21. How many moles of water are formed when 2 moles of H₂ react with 1 mole of O₂?

a) 1

b) 2

c) 3

d) 2✔️

 

22. Which reagent is limiting when 5 moles of H₂ react with 2 moles of O₂?

a) H₂

b) O₂✔️

c) H₂O

d) None

 

23. How many grams of NaOH are required to prepare 1 M solution in 500 mL of water? (Molar mass of NaOH = 40 g/mol)

a) 10 g✔️

b) 20 g

c) 30 g

d) 40 g

 

24. What is the molecular mass of NaCl?

a) 58.5 amu✔️

b) 60 amu

c) 65.5 amu

d) 50 amu

 

25. What is the ratio of nitrogen to hydrogen in ammonia (NH₃) by mass?

a) 14:1

b) 1:3

c) 14:3✔️

d) 1:2

 

26. Which gas has the lowest molar mass?

a) Hydrogen✔️

b) Oxygen

c) Nitrogen

d) Helium

 

27. How many moles of oxygen molecules are present in 64 g of O₂? (O = 16)

a) 1

b) 2✔️

c) 3

d) 4

 

28. What is the empirical formula of benzene (C₆H₆)?

a) CH✔️

b) CH₂

c) C₂H₂

d) C₃H₆

 

29. What is the molar mass of sulfuric acid (H₂SO₄)?

a) 98 g/mol✔️

b) 100 g/mol

c) 90 g/mol

d) 88 g/mol

 

30. Which compound contains 40% carbon, 6.7% hydrogen, and 53.3% oxygen?

a) Glucose

b) Methane

c) Ethanol

d) CH₂O✔️

 

31. What is the percentage of nitrogen in NH₃? (N = 14, H = 1)

a) 82.4%✔️

b) 17.6%

c) 50%

d) 14%

 

32. How many moles are in 100 g of NaOH? (Na = 23, O = 16, H = 1)

a) 2.5✔️

b) 4

c) 1

d) 3

 

33. What is the molecular mass of methane (CH₄)?

a) 16 amu✔️

b) 18 amu

c) 32 amu

d) 44 amu

 

34. Which element has the highest percentage composition in H₂SO₄?

a) Hydrogen

b) Sulfur

c) Oxygen✔️

d) Carbon

 

35. How many atoms are present in 1 mole of H₂ gas?

a) 6.022 × 10²³

b) 1.204 × 10²⁴✔️

c) 3.011 × 10²³

d) 9.033 × 10²³

 

36. What is the mass of 0.25 mole of CO₂?

a) 22 g

b) 11 g✔️

c) 44 g

d) 88 g

 

37. The volume occupied by 1 mole of any gas at STP is:

a) 22.4 L✔️

b) 24 L

c) 18 L

d) 10 L

 

38. Which of the following is an example of a combination reaction?

a) 2H₂ + O₂ → 2H₂O✔️

b) CaCO₃ → CaO + CO₂

c) Zn + HCl → ZnCl₂ + H₂

d) NaCl → Na⁺ + Cl⁻

 

39. What mass of oxygen is required to react with 4 g of hydrogen to form water?

a) 32 g✔️

b) 8 g

c) 4 g

d) 16 g

 

40. What is the limiting reagent when 10 g of H₂ reacts with 20 g of O₂? (H = 1, O = 16)

a) H₂✔️

b) O₂

c) H₂O

d) Both are limiting

 

41. What is the molecular formula of a compound with empirical formula NO₂ and molar mass 92 g/mol?

a) NO

b) N₂O₂

c) NO₂

d) N₂O₄✔️

 

42. What is the volume of 1 mole of oxygen gas at STP?

a) 22.4 L✔️

b) 11.2 L

c) 44.8 L

d) 18 L

 

43. How many grams are in 0.1 moles of H₂SO₄?

a) 9.8 g...