NEET National Eligibility Cum Entrance Test Chemistry Class 11 + 12 Volume I + Volume II

Preface

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!

Table of Contents

Preface

CHAPTER 1

CHAPTER 2

CHAPTER 3

CHAPTER 4

CHAPTER 5

CHAPTER 6

CHAPTER 7

CHAPTER 8

CHAPTER 9

CHAPTER 10

CHAPTER 11

CHAPTER 12

CHAPTER 13

CHAPTER 14

CHAPTER 15

CHAPTER 16

CHAPTER 17

CHAPTER 18

CHAPTER 19

CHAPTER 20

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 ✔️

b) 10 g

c) 8.8 g

d) 12 g

44. Which compound has the highest molar mass?

a) CO₂

b) CH₄

c) NaCl

d) C₆H₁₂O₆ ✔️

45. How many moles of NaCl are in 117 g? (Na = 23, Cl = 35.5)

a) 2 mol ✔️

b) 3 mol

c) 1 mol

d) 0.5 mol

46. What is the percentage of oxygen in CO₂?

a) 72.7% ✔️

b) 44%

c) 32%

d) 55.5%

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

a) 6.022 × 10²³

b) 3.011 × 10²³

c) 1.204 × 10²⁴ ✔️

d) 9.033 × 10²³

48. Which element has the smallest atomic mass?

a) Hydrogen ✔️

b) Helium

c) Oxygen

d) Carbon

49. What is the molar mass of Na₂CO₃? (Na = 23, C = 12, O = 16)

a) 106 g/mol ✔️

b) 100 g/mol

c) 110 g/mol

d) 120 g/mol

50. How many moles of CO₂ are produced when 1 mole of CH₄ is burned?

a) 1 ✔️

b) 2

c) 0.5

d) 4

51. What is the empirical formula of a compound that contains 40% sulfur and 60% oxygen?

a) SO₂ ✔️

b) SO₃

c) S₂O₃

d) S₂O₅

52. Which gas has the highest molar mass?

a) CO₂ ✔️

b) CH₄

c) O₂

d) N₂

53. How many atoms are present in 2 moles of nitrogen gas (N₂)?

a) 6.022 × 10²³

b) 1.204 × 10²⁴ ✔️

c) 3.011 × 10²³

d) 9.033 × 10²³

54. What is the percentage composition of hydrogen in ammonia (NH₃)?

a) 17.6% ✔️

b) 18%

c) 14%

d) 20%

55. How many moles of NaOH are present in 80 g? (Molar mass = 40 g/mol)

a) 2 ✔️

b) 1

c) 4

d) 0.5

56. How many moles of water are formed from the complete combustion of 2 moles of CH₄?

a) 1

b) 2

c) 4 ✔️

d) 8

57. Which element has the highest percentage by mass in Na₂SO₄? (Na = 23, S = 32, O = 16)

a) Sodium

b) Oxygen ✔️

c) Sulfur

d) Hydrogen

58. Which of the following gases follows the Law of Multiple Proportions?

a) O₂ and O₃

b) CO and CO₂ ✔️

c) H₂ and H₂O

d) N₂ and NH₃

59. The molecular formula of ethane is:

a) CH₄

b) C₂H₆ ✔️

c) C₃H₈

d) C₂H₄

60. Which element contributes most to the molar mass of H₂SO₄?

a) Hydrogen

b) Sulfur ✔️

c) Oxygen

d) Sodium

61. How many moles of oxygen are required to burn 1 mole of propane (C₃H₈)?

a) 3

b) 4

c) 5

d) 5 moles ✔️

62. The molecular mass of ammonia (NH₃) is:

a) 17 amu ✔️

b) 18 amu

c) 28 amu

d) 44 amu

63. What is the volume of 2 moles of a gas at STP?

a) 22.4 L

b) 44.8 L ✔️

c) 11.2 L

d) 32 L

64. How many atoms are in 0.25 moles of H₂?

a) 3.011 × 10²³ ✔️

b) 6.022 × 10²³

c) 1.204 × 10²⁴

d) 9.033 × 10²³

65. What is the molar ratio of Na to Cl in NaCl?

a) 2:1

b) 1:1 ✔️

c) 1:2

d) 2:2

66. How many grams are in 0.2 moles of NaOH?

a) 8 g ✔️

b) 10 g

c) 12 g

d) 14 g

67. What is the empirical formula of acetic acid (C₂H₄O₂)?

a) CHO

b) CH₂O ✔️

c) C₂HO

d) CH₄

68. Which law is used to balance chemical equations?

a) Law of Definite Proportions

b) Law of Conservation of Mass ✔️

c) Law of Multiple Proportions

d) Avogadro’s Law

69. How many molecules are present in 1 mole of oxygen (O₂)?

a) 6.022 × 10²³ ✔️

b) 3.011 × 10²³

c) 1.204 × 10²⁴

d) 9.033 × 10²³

70. How many atoms are in 1 mole of water molecules?

a) 6.022 × 10²³

b) 1.807 × 10²⁴ ✔️

c) 3.011 × 10²³

d) 9.033 × 10²³

71. How many moles of NaOH are in 80 g? (Molar mass = 40 g/mol)

a) 1 mol

b) 2 mol ✔️

c) 3 mol

d) 4 mol

72. What is the percentage composition of oxygen in H₂O?

a) 33%

b) 88.9% ✔️

c) 44%

d) 22%

73. Which gas has a molar mass of 32 g/mol?

a) O₂ ✔️

b) CO₂

c) CH₄

d) H₂

74. How many moles of CO₂ are produced from 1 mole of CH₄?

a) 1 ✔️

b) 2

c) 0.5

d) 4

75. How many grams are in 0.5 moles of H₂SO₄?

a) 49 g ✔️

b) 48 g

c) 98 g

d) 25 g

76. What is the molar mass of glucose (C₆H₁₂O₆)?

a) 180 g/mol ✔️

b) 120 g/mol

c) 160 g/mol

d) 200 g/mol

77. How many molecules are present in 0.5 moles of water?

a) 3.011 × 10²³ ✔️

b) 6.022 × 10²³

c) 1.204 × 10²⁴

d) 9.033 × 10²³

78. How many atoms are in 2 moles of sodium (Na)?

a) 1.204 × 10²⁴ ✔️

b) 6.022 × 10²³

c) 9.033 × 10²³

d) 3.011 × 10²³

79. What is the empirical formula of hydrogen peroxide (H₂O₂)?

a) HO ✔️

b) H₂O

c) O₂

d) H₂

80. What is the molar mass of nitrogen gas (N₂)?

a) 14 g/mol

b) 28 g/mol ✔️

c) 32 g/mol

d) 44 g/mol

81. How many moles of H₂O are in 36 g of water?

a) 1 ✔️

b) 2

c) 0.5

d) 4

82. How many grams are in 1 mole of oxygen gas (O₂)?

a) 16 g

b) 32 g ✔️

c) 44 g

d) 18 g

83. How many atoms are in 1 mole of sodium chloride (NaCl)?

a) 1.204 × 10²⁴ ✔️

b) 6.022 × 10²³

c) 9.033 × 10²³

d) 3.011 × 10²³

84. What is the molar mass of CH₄?

a) 16 g/mol ✔️

b) 18 g/mol

c) 32 g/mol

d) 44 g/mol

85. What is the percentage of hydrogen in H₂SO₄?

a) 2% ✔️

b) 3%

c) 4%

d) 5%

86. Which element has the highest atomic mass?

a) Uranium ✔️

b) Hydrogen

c) Oxygen

d) Nitrogen

87. How many molecules are present in 22.4 L of any gas at STP?

a) 6.022 × 10²³ ✔️

b) 3.011 × 10²³

c) 1.204 × 10²⁴

d) 9.033 × 10²³

88. What is the empirical formula of glucose?

a) CH₂O ✔️

b) C₂H₄O₂

c) CHO

d) C₆H₆

89. What is the mass of 2 moles of NaOH?

a) 80 g ✔️

b) 40 g

c) 60 g

d) 20 g

90. Which gas is produced when methane burns in oxygen?

a) CO

b) CO₂ ✔️

c) H₂

d) O₂

91. What is the limiting reagent when 10 g of CH₄ reacts with 20 g of O₂?

a) CH₄ ✔️

b) O₂

c) CO₂

d) H₂O

92. How many moles are in 50 g of NaOH? (Molar mass = 40 g/mol)

a) 1.25 ✔️

b) 0.75

c) 1.5

d) 2

93. What is the molecular formula of a compound with the empirical formula CH₂