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Some Basic Concepts Of Chemistry NEET Questions
1. Philosophy of changing substances into another form is called as _______
a) Physiology
b) Anatomy
c) Alchemy
d) Transformation
Answer: Alchemy
2. Rasopanishada says how the gunpowder mixture is used in war.
a) True
b) False
Answer: False
3. What does the Elixir of life of do?
a) grants immortality
b) cures diseases
c) kills a person
d) cause an incurable disease
Answer: grants immortality
4. The paintings on the walls of Ajanta and Ellora cave were based on ________
a) Varahmihir’s Brihat Samhitha
b) Sushruta Samhita
c) Rasopanishada
d) Charaka Samhita
Answer: Varahmihir’s Brihat Samhitha
5. Seeds of Manhua plant and oil of Eranda were used in making ________
a) cosmetic powder
b) color dye
c) perfume
d) soap
Answer: soap
6. Charaka Samhita is the oldest known book of Ayurvedic in India.
a) True
b) False
Answer: True
7. Patients suffering from AIDS can be helped using which of the following drugs?
a) Cisplatin
b) AZT (Azidothymidine)
c) Taxol
d) Codeine
Answer: AZT (Azidothymidine)
8. What are the basic constituents of matter?
a) Atoms & Molecules
b) Atoms & Moles
c) Molecules & Ions
d) Nuclei & Ions
Answer: Atoms & Molecules
9. What are pure substances classified as?
a) Elements and Atoms
b) Molecules and Compounds
c) Elements and Compounds
d) Atoms and Molecules
Answer: Elements and Compounds
10. When two or more atoms of different elements combine with each other in a fixed ratio, the molecule of a ____ is obtained.
a) Compound
b) Element
c) Atom
d) Ion
Answer: Compound
11. Compounds cannot be separated by chemical methods.
a) True
b) False
Answer: False
12. Point out an example of a compound.
a) Sugar solution
b) Hydrogen
c) Ammonia
d) Sodium
Answer: Ammonia
13. Water is a/an _______
a) Element
b) Compound
c) Pure substance
d) Mixture
Answer: Compound
14. The substances whose compositions are not uniform and different components are mixed are called _______
a) Homogenous substances
b) Heterogeneous substances
c) Pure substances
d) Elements
Answer: Heterogeneous substances
15. A ________ is made up of two or more pure substances which may be in any ratio.
a) Mixture
b) Element
c) Molecule
d) Atom
Answer: Mixture
16. Matter can be divided into two types i.e. mixture and pure substance.
a) True
b) False
Answer: True
17. What is the symbol of the amount of substance’s S.I. unit?
a) K
b) s
c) mol
d) kg
Answer: mol
18. What are the multiples for the prefixes yocto, atto respectively?
a) 10-24, 10-18
b) 10-9, 10-15
c) 10-15, 10-24
d) 10-24, 10-21
Answer: 10-24, 10-18
19. 1Litre = _______ m3.
a) 1000
b) 0.001
c) 1
d) 10
Answer: 0.001
20. What is the difference in units between Kelvin and centigrade scales of temperature?
a) 212.15
b) 32
c) 298
d) 273.15
Answer: 273.15
21. What is the human body temperature in Fahrenheit?
a) 212
b) 98.6
c) 273.15
d) 32
Answer: 98.6
22. Convert 40°C to °F.
a) 104K
b) 313°F
c) 104°F
d) 313K
Answer: 104°F
23. Which of the following may not be a physical property?
a) Odor
b) Color
c) Density
d) Composition
Answer: Composition
24. The observation of __________ properties needs a chemical change to occur.
a) Chemical
b) Physical
c) Extrinsic
d) Intrinsic
Answer: Chemical
25. How many significant figures does 0.057 have?
a) 2
b) 4
c) 3
d) 0
Answer: 2
26. How many significant figures does 63180 have?
a) 5
b) 4
c) 1
d) 2
Answer: 4
27. The exact value is 150m. A students record it as 140.1m in 1st turn and 140.8m in the 2nd turn. Comment his/her recordings.
a) precise
b) accurate
c) neither precise nor accurate
d) both precise and accurate
Answer: precise
28. The exact value is 150m. A students record it as 149.1m in 1st turn and 150.8m in the 2nd turn. Comment his/her recordings.
a) precise
b) accurate
c) neither precise nor accurate
d) both precise and accurate
Answer: accurate
29. Multiply 1.2 and 3.91. Obtain the result as per the rules of significant figures.
a) 4.692
b) 4.69
c) 5
d) 4.7
Answer: 4.7
30. How many significant figures are there in 60.6?
a) 4
b) 2
c) 3
d) 1
Answer: 3
31. Write 6354000000 in scientific notation.
a) 6.354 x 109
b) 6354 x 106
c) 0.64 x 1010
d) 6354000 x 103
Answer: 6.354 x 109
32. _________ is referred to as the closeness of different measurements for the same quantity.
a) Accuracy
b) Precision
c) Analysis
d) Dimension
Answer: Precision
33. Who proposed the Law of Definite Composition?
a) Joseph Proust
b) Lorenzo Romano
c) Joseph Louis
d) Antoine Lavoisier
Answer: Joseph Proust
34. Law of Definite Composition is also known as ________
a) Law of Multiple Proportions
b) Avogadro’s Law
c) Law of Definite Proportion
d) Law of Conservation of Mass
Answer: Law of Definite Proportion
35. The volumes of hydrogen & oxygen when combined bear a simple ratio of 2:1.This is explained by ________
a) Law of Multiple Proportions
b) Avogadro’s Law
c) Law of Definite Proportion
d) Gay Lussac’s Law of Gaseous Volumes
Answer: Gay Lussac’s Law of Gaseous Volumes
36. Who proposed that equal volumes of all gases at the same temperature & given pressure should contain an equal number of molecules?
a) Antoine Lavoisier
b) Joseph Proust
c) Avogadro
d) Joseph Louis
Answer: Avogadro
37. Which of the following is not a law of chemical combination?
a) Law of Multiple Proportions
b) Avogadro’s Law
c) Law of Definite Proportion
d) Law of Conservation of volume
Answer: Law of Conservation of volume
38. Which of the following may be an incorrect statement?
a) Law of Definite Composition is also known as Law of Definite composition
b) Mass can neither be created nor destroyed is Law of Conservation of Volume
c) Antoine Lavoisier conducted many experiments regarding combustion
d) Five basic laws are required to govern the combination of elements to form compounds
Answer: Mass can neither be created nor destroyed is Law of Conservation of Volume
39. How many basic laws are required to govern the combination of elements to form compounds?
a) 6
b) 5
c) 4
d) 1
Answer: 5
40. Who proposed Law of Conservation of Mass?
a) Antoine Lavoisier
b) Joseph Proust
c) Lorenzo Romano
d) Joseph Louis
Answer: Antoine Lavoisier
41. Which of the following may not be explained by Dalton’s atomic theory?
a) reason for combining atoms
b) conservation of mass
c) chemical philosophy
d) indivisible atoms
Answer: reason for combining atoms
42. Law of conservation of mass isn’t explained in Dalton’s atomic theory.
a) True
b) False
Answer: False
43. What is 1 Dalton?
a) a unified mass unit, 1.360539040(20)×10−27kg
b) a unified mass unit, 1.640539040(20)×10−27kg
c) a unified mass unit, 1.660539040(20)×10−27kg
d) a unified mass unit, 1.660539040(20)×10−27kg
Answer: a unified mass unit, 1.660539040(20)×10−27kg
44. Could Dalton’s atomic theory explain the laws of chemical combinations?
a) No
b) Yes
c) Only a few
d) Except one
Answer: Yes
45. They are no limitations to Dalton’s atomic theory.
a) True
b) False
Answer: False
46. All atoms of a given element have identical __________ including identical _________
a) Properties, mass
b) Weight, volume
c) Volume, properties
d) Temperature, pressure
Answer: Properties, mass
47. According to Dalton’s Atomic Theory, matter consists of indivisible _______
a) Molecules
b) Atoms
c) Ions
d) Mixtures
Answer: Atoms
48. Atoms of different elements differ in mass.
a) True
b) False
Answer: True
49. A sample of carbon that contains 70% carbon-12 and 30% carbon-14. What do you think is the average atomic mass of this sample?
a) 14.5
b) 14.14
c) 14
d) 12
Answer: 14
50. ______ is the sum of atomic masses of the elements present in a molecule.
a) Average atomic mass
b) Atomic mass
c) Gram formula mass
d) Molecular mass
Answer: Molecular mass
51. What’s the molecular mass of carbon dioxide?
a) 43
b) 28
c) 44
d) 40
Answer: 44
52. What’s the formula mass of NaCl?
a) 23 u
b) 35.5 u
c) 58 u
d) 58.5 u
Answer: 58.5 u
53. Calculate the molecular mass of sucrose(C12H22O11) molecule?
a) 342 amu
b) 343 amu
c) 341 amu
d) 340 amu
Answer: 342 amu
54. As, per the current system, carbon-12 has been taken as the standard for measuring atomic masses.
a) True
b) False
Answer: True
55. What is the mass of hydrogen in terms of amu?
a) 1.0020 amu
b) 1.0180 amu
c) 1.0070 amu
d) 1.0080 amu
Answer: 1.0080 amu
56. What is the abbreviation of amu?
a) Atomic matter unit
b) Atomic mass unified
c) Atomic mass unit
d) At mass unity
Answer: Atomic mass unit
57. 12.044 x 1023 atoms of oxygen contains
a) 1 mole of oxygen
b) 2 moles of oxygen
c) 3 moles of oxygen
d) 4 moles of oxygen
Answer: 2 moles of oxygen
58. If one mole of ammonia contains “y” number of particles, then how many particles do 1 mole of glucose contain?
a) 2y
b) 0.5y
c) 3y
d) y
Answer: y
59. What’s the number of particles in 10 moles of hydrochloric acid?
a) 6.022 x 1022 particles
b) 6.022 x 1023 particles
c) 6.22 x 1023 particles
d) 3.22 x 1022 particles
Answer: 6.022 x 1022 particles
60. Which of the following statement is correct?
a) The value of Avogadro’s number is 6.022×1022 atoms
b) One molecule of any substance contains Avogadro’s number of particles
c) One mole is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of the carbon atom
d) 1 u is not equal to Ma/NA
Answer: One mole is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of the carbon atom
61. One mole of sucrose contains how many grams of sucrose?
a) 342g
b) 343g
c) 341g
d) 340g
Answer: 342g
62. 1 mole of ammonia is of 17 g. Then what is the mass of 0.3 moles of ammonia?
a) 21g
b) 2.1g
c) 17g
d) 1g
Answer: 2.1g
63. According to S.I. the system, ______ was used to measure the amount of substance.
a) mole
b) weight machine
c) weight
d) mass
Answer: mole
64. What’s the number of entities or particles together in mole concept known as?
a) Boltzmann constant
b) Avogadro’s number
c) Universal gas constant
d) Reynold’s number
Answer: Avogadro’s number
65. The molecular formula of a compound is C6H12O6. What’s the empirical formula for this compound?
a) C6H12O6
b) CHO
c) C2H6O2
d) CH2O
Answer: CH2O
66. A compound consists of 52.17% of carbon, 13.04% of hydrogen and 34.78% of oxygen. Find the molecular formula if the given molecular weight of the compound is 46g.
a) C2H5OH
b) C2H6
c) C6H12O6
d) CH2O
Answer: C2H5OH
67. Which of the following cannot be a molecular formula for an empirical formula HO?
a) H2O
b) H2O2
c) HO
d) HO2
Answer: H2O2
68. In glucose simplest ratio between C, H and O is ________
a) 6:12:6
b) 3:4:3
c) 1:2:1
d) 2:3:2
Answer: 1:2:1
69. Which of the following is true regarding molecular formula?
a) actual whole numbered ratio
b) rational numbered ratio
c) simplest possible whole numbered ratio
d) the same as the empirical ratio
Answer: actual whole numbered ratio
70. Which of the following cannot be an empirical formula?
a) NH3
b) C5H10
c) H2O
d) NaCl
Answer: C5H10
71. A _______ formula represents a whole number ratio to the simplest form.
a) Molecular
b) Empirical
c) Simpler
d) Shorter
Answer: b
72. Even without knowing the mass percent of each element, we can calculate the empirical formula.
a) True
b) False
Answer: b
73. Calculate the mass percent of magnesium in the formation of magnesium oxide.
a) 0.3
b) 1.5
c) 0.67
d) 0.6
Answer: 0.6
74. A solution contains 8 moles of solute and the mass of the solution is 4 kg. What’s the molality of this solution?
a) 5 mol/kg
b) 8 mol/kg
c) 4 mol/kg
d) 0.5 mol/kg
Answer: 0.5 mol/kg
75. In a container, there are 4 moles of nitrogen, 3 moles of oxygen and 7 moles of hydrogen; find out the mole fraction of oxygen in this reaction.
a) 0.2143
b) 0.2142
c) 0.1234
d) 0.2434
Answer: 0.2143
76. Find the amount of carbon dioxide produced by the combustion of 20g of methane.
a) 44g
b) 20g
c) 66g
d) 22g
Answer: 66g
77. What’s the balanced equation of CO2 + H2O → C6H12O6 + O2?
a) CO2 + H2O → C6H12O6 + O2
b) 6 CO2 + 6 H2O → C6H12O6 + 6 O2
c) 6 CO2 + 6 H2O → C6H12O6 + 2 O2
d) 3 CO2 + 2H2O → C6H12O6 + O2
Answer: 6 CO2 + 6 H2O → C6H12O6 + 6 O2
78. In a particular reaction, one of the reactants limits the number of products formed. That is called as _______
a) Limiting reagent
b) Limiting product
c) Excessive reagent
d) Excessive reactant
Answer: Limiting reagent
79. Which of the following is not true regarding balanced chemical equations?
a) They contain the same number of atoms on each side
b) Electrons are also balanced
c) An equal number of molecules on both the side
d) Follows the law of conservation of mass
Answer: An equal number of molecules on both the side
80. Which of the given reactions are counted as balanced reactions?
a) H2 + O2 → 2H2O
b) 4Al + 3O2 → 2Al2O3
c) Mg(OH)2 + 2HNO3 → 2Mg(NO3)2 + 2H2O
d) N2 + 3H2 → NH3
Answer: 4Al + 3O2 → 2Al2O3
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