chemistry mcqs handouts

CHEMICAL BASICS PREPARED BY

EXTRA MCQS HANDOUT 1 OSAMA HASAN

1 | P a g e o u t o f | 1

PREPARED BY OSAMA HASAN

1. How many protons, neutrons and electrons are there in an atom of 19F (Z = 9)? A) 9 protons, 9 neutrons and 9

electrons B) 19 protons, 10 neutrons and

19 electrons C) 9 protons, 10 neutrons and 9

electrons 2. How many protons, neutrons and electrons are there in an atom of 22Ne (Z = 10)? A) 10 protons, 10 neutrons and

10 electrons B) 22 protons, 12 neutrons and

22 electrons C) 10 protons, 12 neutrons and

10 electrons 3. Which one of the following has 19 protons, 20 neutrons and 19 electrons? A) 39K (Z=19) B) 41K (Z=19) C) 40Ca (Z=20) 4. Identify the isotope that has 5 protons, 10 neutrons and 5 electrons. A) 20Ne B) 10B C) 30P 5. Which one of the following has 17 protons, 18 neutrons and 17 electrons? A) 35Cl (Z=17) B) 32S (Z=16) C) 40Ar (Z=18) 6. If copper has an atomic number of 29, Cu-63 and Cu-65 both have? A) 29 protons & 29 electrons B) 29 protons & 34 neutrons C) 36 neutrons & 29 electrons 7. If oxygen has an atomic number of 8, O-16, O-17 and O-18 all have? A) 8 protons & 8 neutrons B) 8 Protons & 8 electrons C) 9 Neutrons and 8 electrons 8. Express the number 0.0000000723 in scientific notation. A) 7.23 x 10-7 B) 7.23 x 10-8 C) 7.23 x 10-9 9. If the Br-Br bond length in Br2 (g) is 228 pm, what is the bond length in Å? A) 0.0228 Å B) 22800 Å C) 2.28 Å 10. An enzyme reaction was carried out in 500 µL vessel. What is the volume of vessel? A) 5.00 x 10-1 ml B) 5.00 x 10-4 ml C) 5.00 x 10-7 ml 11. A gold coin with a mass of 96.5 g is placed in exactly 100 ml of water. If 5 ml of water is displaced, then the density gold of coin is? A) 1.02 g/ml B) 19.3 g/ml C) 0.0518 g/ml 12. The density of bismuth is 8.90 g/cm3. What would be the mass of 1 in3 of Bi? A) 3.50 g B) 22.6 g C) 146 g

CHEMICAL LANGUAGE PREPARED BY


1 | P a g e o u t o f | 3


1. If carbon is burnt in limited supply of oxygen, then the product is rich in?

A) Carbon monoxide B) Carbon dioxide C) Both have equal

volumes

D) No such gas is

evolved

2. A mole of magnesium and a mole of iron have same number of?

A) Atoms B) Molecules C) Masses D) Protons

3. A mole of magnesium and a mole of iron have different?

A) Masses B) Atoms C) Subatomic

particles

D) Both (a) and (c)

4. The mass of 1.0 x 1023g of Magnesium atoms id about?

A) 2.4 x 10-23 g B) 4.0 x 10

-23 g C) 2.4 g D) 4.0 g

5. Which of the following is a reasonable value for the number of atoms in 1.00 f of Helium?

A) 0.25 B) 1.51 C) 1.51 x 10-23 D) 1.51 x 10

23

6. Which of the following is the reasonable value for the mass of a calcium atom?

A) 6.7 x 10-23 g B) 40.1 g C) 6.7 x 10

-23 u D) 6.7 x 10

23 u

7. Which of these compounds contains the greatest mass of sulphur per gram of compound?

A) BaSO4 B) Li2SO4 C) Na2SO4 D) PbSO4

8. Which of these compounds have the greatest percent nitrogen by mass?

A) NH4SO4 B) NH4NO3 C) NH4I D) All have equal

9. You have available 10.0 g of each of the following solutes. Which among them, when used to

prepare 100.ml solution will yield the solutions of greatest molarity?

A) CO(NH2)2 B) C6H12O6 C) CH3CH2OH D) NH3

10. How many moles of nitrogen atoms are present 10.62 g of Nitrogen gas?

A) 0.758 mole B) 0.379 mole C) 1.516 mole D) 2.636 moles

11. How many moles of hydrogen are present in 8.8 g of Methane (CH4)?

A) 0.55 moles B) 1.1 moles C) 2.2 moles D) 0.2 moles

12. How many atoms of oxygen are present in 1 m mole of Ozone (O3)?

A) 1.81 x 1021 B) 1.81 x 10

27 C) 6.2x 10

29 D) 6.2 x 10

20

13. How many hydrogen atoms are present in 56.8 moles of Hydrogen gas?

A) 3.42 x 1025 B) 6.84 x 10

25 C) 6.84 x 10

23 D) 7.04 x 10

25

14. Which sample contains greater number of atoms?

A) 1 g Phosphorous B) 1 g of Iron C) 1 g Krypton D) 1 g Uranium

15. Calculate the mass of a single molecule of ammonia?

A) 17 g B) 2.83 x 10-23 g C) 1.03 x 10

25 g D) 2.82 x 10

23 g



2 | P a g e o u t o f | 3


16. A compound of nitrogen and hydrogen contains 87.4% N. What is the empirical formula of

the compound?

A) NH2 B) N2H4 C) NH3 D) None

17.A compound composed of Chromium and Oxygen contains 68.42% Cr. What is the formula of

the compound?

A) Cr2O3 B) Cr4O3 C) Cr4O6 D) Cr3O2

18. Sodium metal of mass 0.584 reacts with Phosphorous to form 0.846 g of a pure compound.

What is the empirical formula of the compound?

A) NaP3 B) NaP C) Na3P D) None

19. When 8.64 g of vanadium is combined with oxygen, 15.4 g of a compound is formed. What is

the formula of this compound?

A) VO3 B) V2O5 C) V4O5 D) V3O5

20. The molecular mass of terephthalic acid is 166 g and its empirical formula is C4H3O2. What

is the molecular formula of the acid?

A) C12H9O6 B) C4H3O2 C) C16H12O8 D) C8H6O4

21. The molecular mass of ethyl acetate is 88 g and its empirical formula C2H4O. What is the

molecular formula of the compound?

A) C2H4O B) C4H8O2 C) C6H12O3 D) C8H16O4

22. How many atoms of Vanadium can be extracted from 4 moles of vanadinite

(PbO)9(V2O5)3PbCl2?

A) 24 B) 8 C) 12 D) 6

23. How many moles of Boron can be extracted from 2.5 moles of Borax, Na2B4O7.10H2O?

A) 2.5 B) 4 C) 10 D) 100

24. How many moles of carbon monoxide are produced when 0.488 moles of SnO2 react with

excess of carbon? The equation of the reaction is:

SnO2 + 2 C

>Sn + 2 CO

A) 0.844 mole B) 0.422 mole C) 0.211 mole D) 0.122 mole

25. How many moles of carbon are required to react 1.88 moles of SnO2 completely? The

equation of the reaction is:

SnO2 + 2 C

>Sn + 2 CO

A) 1.88 moles B) 0.94 mole C) 1.41 mole D) 3.76 mole

26. How many moles of nitric acid will be prepared from 8 moles of NO2 and 3 moles of H2O?

A) 16 moles B) 5.33 moles C) 6 moles D) 10 moles



3 | P a g e o u t o f | 3


For Questions 27-29, consider the following chemical equation:

5 �a�3 + �a�O3

>3�a2O + 8�2

27. If 15 moles of NaN3 and 4 moles of NaNO3 react according to the following chemical

equation, how many moles of N2 are produced?

A) 32 moles B) 2.7 moles C) 24 moles D) 27 moles

28. Predict that if 2 moles of N2 are produced, how many moles of Na2O will be produced?

A) 0.75 moles B) 0.067 moles C) 5.3 moles D) 12 moles

29. Predict that if 0.75 moles of Na2O are produced, how many moles N2 of will be produced?

A) 0.28 moles B) 0.094 moles C) 18 moles D) 2 moles

For Questions 30-31, consider the following chemical equation:

6 �a + Al2O

> 2 Al + 3 �a2O

30. How many moles of Al are produced from 1.00 mole of each reactant?

A) 1 mole B) 0.333 mole C) 0.167 mole D) 2 mole

31. How many moles of Al are produced from 3 moles of each reactant?

A) 6 moles B) 0.5 mole C) 1 mole D) 9 mole

32. How many moles of OH- ions are contained in 125 ml of 0.625M Ba(OH)2?


33. How many moles of H+ ions are presented in 125 ml of an aqueous solution that is 0.625 M

oxalic acid, H2C2O4?


34. Combustion analysis of 12 mg sample of ibuprofen produced 9.50 mg of water. What is the

percentage of hydrogen in ibuprofen?

A) 4.40% B) 17.6% C) 8.80% D) 11.11%

35. Calculate the mass of sodium sulphate required to make 2.50 L of 1.09M sodium sulphate,

Na2SO4.

A) 155g B) 387g C) 62g D) 142g

36. Calculate the volume of 0.755 M Na2S2O3 that should be used to prepare 15 L of 0.319 M

Na2S2O3.

A) 19.9 L B) 4.79 L C) 6.34 L D) 12.7 L

CHEMICAL TECHNIQUES PREPARED BY


1 | P a g e o u t o f | 4


1. Which of the following is not a gas at room temperature and normal pressure? A) Fluorine B) Chlorine C) Bromine D) All are gases

2. Which of the following is not a gas at room temperature and normal pressure?

A) Argon B) Iodine C) Neon D) All are gases

3. Which of the following represent the elements in most stable form at 25°C and 1atm?

A) Br2 (l) and I2 (s) B) Br2 (g) and I2 (g) C) Br2 (l) and I2 (l) D) None

4. An aqueous solution labelled “Potassium dichromate” contains the ions?

A) K+, Cr

3+ and OH

- B) K

+ and Cr2O7

2- C) K

+ and CrO4

2- D) 2 K

+ and CrO4

2-

5. Which of the following is an intensive property of a substance?

A) Volume B) Colour C) Mass D) None

6. Which of the following is an intensive property of a substance?

A) Volume B) Density C) Energy Content D) Matter

7. Which of the following is the example of solid-solid separation methods?

A) Destructive

Distillation

B) Melting C) Wind Winnowing D) All of the above

8. Separation of alum crystals from solution takes place according to the process of?

A) Crystallization B) Filtration C) Melting D) Heating

9. Alum is prepared from the mother liquor by?

A) Crystallization B) Sublimation C) Melting D) Boiling

10. Conversion of hard waters into soft waters is a chain of process. It also includes?

A) Flocculation B) Distillation C) Decantation D) Crystallization

11. Sodium Chloride is commonly known as Table salt. It could be separated from sea water by?

A) Flocculation B) Distillation C) Decantation D) Crystallization

12. Froth Floatation and Induced gas floatation are the examples of which type of separation

technique?

A) Decantation B) Solid Phase

Extraction

C) Dissolved Air

Floatation

D) Flocculation

13. Water waste from a fast food restaurant has oil traces. A student has been assigned with the

task to separate the oil from water. He would go for which of the following separation process?

A) Filtration B) Distillation C) Decantation D) Solid Phase

Extraction

14. A researcher needs to extract oil from oil seeds. Hw may use which of the following process?



2 | P a g e o u t o f | 4


A) Expeller Press B) n-hexane C) SCFE D) All

15. For the situation provided in Q14. Which of the following will have highest efficiency?

A) SCFE B) n-hexane C) Expeller Press D) All have the same

16. Two liquids of different density have been mixed properly. A student has to separate them.

Which method will opt for?

A) Distillation B) Centrifugation C) Flocculation D) None

17. In an advanced industry, a workman mistakenly mixed water with alcohol. By which method

could he separate this mixture?

A) Centrifugation B) Vacuum

Distillation

C) Fractional

Freezing

D) Fractional

Distillation

18. Kerosene oil is a by-product of crude oil which yields petroleum. It is separated from the

fraction by?

A) Fractional

Distillation

B) Critical Fluid

Extraction

C) Decantation D) None

19. Electrophoreses separates the mixture by which method?

A) Electron capturing B) Electric Current C) Electric Charge D) Both (B) and (C)

20. The separation process that separates mixture due to difference in densities is/are?

A) Flocculation B) API oil-water

separator

C) Centrifugation D) All of them

21. Melting point is the basic separating characteristic for which of the following processes?

A) Fractional

distillation

B) Fractional freezing C) Fractional boiling D) Fractional melting

22. Which of the following chloride is insoluble?

A) Silver Chloride B) Sodium Chloride C) Iron Chloride D) Aluminium

Chloride

23. Which of the following sulphates is insoluble?

A) Sodium Sulphate B) Beryllium Sulphate C) Lithium Sulphate D) Calcium Sulphate

Q24. Which of the following hydroxide is insoluble?

A) Calcium Hydroxide B) Sodium Hydroxide C) Aluminium

Hydroxide

D) Both (A) and (C)

25. Which of the following carbonate is insoluble?

A) Calcium Carbonate B) Sodium Carbonate C) Potassium

Carbonate

D) Ammonium

Carbonate



3 | P a g e o u t o f | 4


26. Which of the following is insoluble?

A) Sodium Nitrate B) Ammonium Nitrate C) Potassium Nitrate D) None

27. The soluble chloride is?

A) Silver Chloride B) Potassium Chloride C) Mercury Chloride D) Lead Chloride

28. The soluble sulphate is?

A) Calcium Sulphate B) Barium Sulphate C) Sodium Sulphate D) Lead Sulphate

29. Sugar is dissolved in different water solutions, at following temperature:

Solution I Solution II Solution III IV

101°C 4°C 10°C -10°C

Which solution will have the maximum amount of dissolved sugar?

A) Solution IV B) Solution III C) Solution II D) Solution I

30. Hydrogen Chloride is dissolved in different water solutions, at following temperature:

Solution I Solution II Solution III IV

1 atm 761 torr 769 mm of Hg 101.300 Pa

Which solution will have the maximum amount of dissolved Hydrogen Chloride?

A) Solution IV B) Solution III C) Solution II D) Solution I

31. A gas is exposed to HCl gas container, white fumes are formed. The gas may be?

A) Chlorine B) Hydrogen Sulphide C) Carbon dioxide D) Ammonia

32. White precipitates are formed when a gas is passed through lime water. The gas may be?


33. A yellowish green gas has an irritating odour. The gas may be?


34. A laboratory attendant accidently dropped AgNO3 in an unknown gas’s beaker. White

precipitates are formed. The gas may be?

A) CO2 B) HCl C) NH3 D) CO

35. In a laboratory, several beakers of different gases are arranged. One of the beakers smells like

rotten eggs. The gas may be?

A) Cl2 B) H2 C) SO2 D) H2S

36. In a laboratory, a student accidently removed the lid of an unknown filled gas. The vicinity air

became reddish brown. The gas may be?

A) NO B) N2 C) N2O D) SO2

37. The flame test of Sodium salt is?

A) Silver B) White C) Yellow D) Green

38. Violet is the colour observed in which salt’s flame test?



4 | P a g e o u t o f | 4


A) Lead B) Potassium C) Beryllium D) Chromium

39. The flame test of Copper results in which colour?

A) Red B) Green C) Blue D) Both (B) and (C)

40. Smell of vinegar is smelt when dilute HCl is added to an unknown salt. The salt may have

which ion?

A) Acetate B) Carbonate C) Bicarbonate D) Sulphide

For Question 41-45 consider the following case:

Concentrated H2SO4 is added to an unknown salt. And the solution is then heated. Fumes are

evolved.

41. The salt contains the Chlorine anion if the fumes are __________ coloured.

A) White B) Brown C) Violet D) Colourless

42. The colourless fumes are of?

A) HCl B) Cl2 C) SO2 D) Both (A) and (B)

43. The fumes if exposed to a chemical would turn white. The chemical is?

A) AgCl B) HNO3 C) NH4OH D) AgNO3

44. The salt might contain Bromine anion if the fumes are __________ coloured.


45. The salt might contain Iodine anion if the fumes are __________ coloured.


PERIODIC TABLE PREPARED BY


1 | P a g e o u t o f | 3


1. Which transition element has no electrons in its outer most sub shell?

A) Nickel (Z=28) B) Palladium (Z=46) C) Platinum (Z=78) D) None

2. “One-half the distance between the nuclei of adjacent atoms in a solid metal” is called?

A) Covalent Radius B) Metallic Radius C) Ionic Radius D) Both (A) and (B)

3. Arrange the following elements in order of increasing atomic radius:

Mg Si S

I II III

A) III<II<I B) II<I<<III C) I<III<II D) I<II<III

4. Arrange the following elements in order of decreasing atomic radius:

As N P

I II III

A) I>II>III B) II>III>I C) III>I>II D) I>III>II

5. The first ionization energy of an atom is always?

A) Highest B) Average C) Lowest D) It varies

6. The elements with smaller number of electrons in their outermost shell are?

A) Metals B) Non-Metals C) Metalloids D) Inert gases

7. The elements with greater number of electrons in their outermost shell are?

A) Metals B) Non-Metals C) Metalloids D) Inert gases

8. Elements with more than __________ protons tend to be radioactive.

A) 92 B) 83 C) 80 D) 72

9. Among the following, which element has smallest atomic radius?

A) Be B) Al C) P D) I

10. Among the following, which element has the largest atomic radius?

A) Be B) Al C) P D) I

11. The representive element with the smallest atomic radius in the periodic table is?

A) He B) F C) Ne D) O

12. The element with the largest atomic radius is?

A) Ra B) Ca C) Fr D) Cs

13. What will affect the atomic radius more?

A) Nuclear Charge B) Electron Shell C) Both will be equal D) None

14. Fluorine gained an electron from a metal atom. The atomic radius is expected to?

A) Increase B) Decrease C) Remain same D) None



2 | P a g e o u t o f | 3


15. Calcium donated two electrons to a non-metal atom. Its atomic radius will?

A) Increase B) Decrease C) Remain same D) None

16. The outermost valence electrons are equidistant in atoms of two different elements. They are

supposed to have same?

A) Atomic Radius B) Ionization Potential C) Electron Affinity D) None

17. The nuclear charge of two atoms could only be same when they have equal?

A) Electrons B) Neutrons C) Protons D) Both (B) and (C)

18. Removing electrons is easiest from?

A) f-shell B) d-shell C) p-shell D) None

19. The element with the least value of ionization potential is?

A) Rb B) Cs C) Mg D) Fr

20. The element with the highest value of ionization potential is?

A) Al B) O C) F D) Ne

21. The distance of valence electrons of atom A is twice that of the electrons of atom B. The

expected ionization potential of A would be

A) 1/2 B) 1/4 C) twice D) Can’t be told

22. Elements with stable electronic configuration have _________ values of electron affinity.

A) Higher B) Lower C) Zero D) Moderate

23. The highest value of electron affinity has been calculated for?

A) F B) Cl C) Br D) I

24. Large values of electron affinity show that element is?

A) Dehydrating Agent B) Hydrating Agent C) Reducing Agent D) Oxidizing Agent

25. Increase in atomic radius, makes the value of electron affinity get?

A) Lower B) Higher C) It fluctuates D) None

26. Which of the following has the smallest value for electron affinity?

A) Na B) B C) Li D) O

27. Which of the following has the largest value for electron affinity?

A) Na B) B C) Li D) O

28. The highest value for Electronegativity is?

A) 5 eV B) 4 eV C) 3 eV D) 2 eV



3 | P a g e o u t o f | 3


29. Increase in atomic size, causes the value of Electronegativity become?

A) It doesn’t matter B) Larger C) Smaller D) None

30. The most electronegative element in the periodic table is?

A) F B) Cl C) Br D) I

31. The least electronegative element in the periodic table is?

A) Ra B) Ca C) Cs D) Fr

32. The most electronegative among the following elements is?

A) Ca B) P C) I D) Si

33. The least electronegative among the following elements is?

A) I B) Be C) K D) O

34. The lowest ionization energy would be found with the least _______ atom.

A) Lowest Radius B) Largest Radius C) Electropositive D) Electronegative

STATES OF MATTER PREPARED BY


1 | P a g e o u t o f | 5


1. The Kinetic Molecular Theory explains which dimension of properties of a matter? A) Chemical B) Physical C) Molecular D) Kinetics

2. The molecules of a gas are in such a rapid motion that they seem to resist __________ forces.

A) Attractive B) Repulsive C) Gravitational D) Both (A) and (B)

3. The speed and direction of motion of any given molecule are at all times __________?

A) Same B) Different C) Predictable D) Unpredictable

4. The molecules of a cold sample of gas moves __________ than those of hot sample.

A) Equally B) More fast C) More slowly D) Can’t be predicted

5. Molecules moving at different speeds have different?

A) Acceleration B) Kinetic Energy C) Both (A) and (B) D) None

6. The density of air decreases when the height above the earth’s surface is?

A) Decrease B) Increased C) It doesn’t matter D) It’s constant

7. 1 mm of Hg is equals to how many mm of water?

A) 13.6 B) 13.2 C) 100 D) 10

8. Four containers have gas with the following pressures:

745 mm of Hg 762 torr 75 cm Hg 735 torr

I II III IV

Which has the least pressure enclosed?

A) IV B) III C) II D) I

9. For the information given in 8. Which container carries the maximum pressure?

A) III B) IV C) I D) II

10. What is the pressure drop below atmospheric pressure, during the inspiration of air to lungs?

A) 3 torr B) 3 atm C) 3 Pa D) All of the above

11. What is the total pressure, during the expiration of air from lungs?

A) 763 Pa B) 3 mm of Hg C) 763 mm of Hg D) Both (B) and (C)

12. The volume of air that is moved in and moved out, to and from the lungs during respiration is

called “Tidal Volume”. What is its value for a normal person?

A) ½ litre B) 0.5 cm3 C) 1 dm

3 D) It’s not a constant

13. The volume of a gas in a cylinder is 2.00 L at 398 torr. The piston is moved to increase the

gas pressure to 5.15 atm. Which of the following is the reasonable value for volume?

A) 0.20 L B) 0.40 L C) 1.00 L D) 16.0 L



2 | P a g e o u t o f | 5


14. A gas is enclosed in a 10.2 L tank at 1208 torr. Which of the following is a reasonable value for the pressure when the gas is transferred to a 30.0 L tank?

A) 0.40 atm B) 25 lb/in2 C) 400 mm of Hg D) 3600 torr

15. For each Celsius degree rise in temperature, the volume of a gas expands by 1/273 of it

volume at?

A) Initial temperature B) 25 °C C) 0°C D) 0 K

16. For Avogadro’s law, the gases must be?

A) Non-reacting B) Inert C) At same

Temperature and

Pressure

D) None of these

17. Density of gases, as compared to liquids and solids is?

A) More B) Equal C) Less D) It varies

18. Which of the following has the greatest density?

A) H2 at 100°C, 745

torr

B) He at STP C) CH4 at -10°C

and 765 torr

D) All have equal

densities.

19. A sample of nitrogen occupies a volume of 2.50 L at -120°C and constant pressure. To which

of the following approx. temperatures should the gas be brought in order to double its volume?

A) -240°C B) -60°C C) -12°C D) 30°C

20. When water freezes at 0°, its volume expands about?

A) 9% B) 15% C) 4% D) It remains constant

21. The hydrated crystals that lose the water of crystallization on exposure to air at ordinary

temperature are called?

A) Hydroscopic B) Deliquescent C) Efflorescent D) Both (A) and (B)

22. The crystals that absorb water from air and become wet are called?

A) Hydroscopic B) Deliquescent C) Efflorescent D) Both (A) and (B)

23. At standard conditions, the number of molecules of a gas in a cubic metre is?

A) 3 x 1025 B) 6.02 x 10 C) 3 x 10

-25 D) 3 x 10

-10

24. The molar volume occupied by one mole of any gas at N.T.P is?

A) 22.4 dm3 B) 24.46 dm

3 C) 2.05 dm

3 D) None

25. The molecules to which water molecules are attracted are called?

A) Hygroscopic B) Hydroscopic C) Hydrophilic D) None

26. Dalton’s law is applicable to which set of gases?

A) O2 and N2 B) He and Xe C) Cl2 and H2 D) Both (A) and (C)



3 | P a g e o u t o f | 5


27. Sublimation is a process in which solid directly changes to gaseous state without being

converted into liquid. Such type of a phase change occurs in solids due to?

A) High Vapour

Pressure

B) Very Low

Melting Point

C) High Boiling

Point

D) Both (A) and (B)

28. On reducing the pressure, what change is expected to be observed in a system of gases?

A) Collisions will

become faster

B) Molar Masses

will be reduced

C) Gas density will

decrease.

D) No Change

29. Honey is viscous and water is mobile. This could be due to the difference in?

A) Molecular size B) Nature of liquid C) Temperature D) Pressure

30. Viscosity and Surface tension are examples of which type property?

A) Colligative B) Additive C) Constitutive D) Intensive

31. Vapour pressure is a __________ property of the matter.

A) Colligative B) Additive C) Constitutive D) Intensive

32. Volumes of gases could highly be affected by changes in?

A) Temperature B) Heat C) Pressure D) Area occupied

33. The mass of atmospheric layer on human body at sea level is about?

A) 14.7 psi B) 29.92 in. Of Hg C) 1.36 mm of water D) Both (A) and (B)

34. The tires of automobiles are filled with air until the gauge shows the pressure of about?

A) 28 psi B) 42.7 psi C) Both (A) and (B) D) None

35. 1 mole of a liquid occupies the volume of about?

A) 1 cm3 to 10 cm

3 B) 10 cm

3 to 100cm

3 C) 1 dm

3 to 10 dm

3 D) 10 dm

3 to 100dm

3

36. As compared to gases, diffusion in liquids is?

A) Faster B) Slower C) Equal D) It varies

37. For the molecules of a liquid at surface, there is resultant attractive force acting?

A) Sideward B) Upward C) Downwards D) All forces are in

equilibrium

38. The surface tension of water as compared to most of the organic liquids is?

A) Higher B) Lower C) Equal D) It varies

39. Which state has the highest degree of order?

A) Plasma B) Solid C) Liquid D) Gases

40. The dispersion forces act as the principal forces in which system of crystals?

A) Ionic B) Covalent C) Metallic D) Molecular



4 | P a g e o u t o f | 5


41. Dry ice is an example of which system of crystals?


42. On increasing the concentration of solute in a solution, the vapour pressure is/remains?

A) Same B) Lowered C) Increased D) It’s a constant

43. The hardest system of crystals is?


44. Which crystal system could be used in making electrical wires?


45. Which crystal system exhibits the property of indefinite growth of crystals?


46. The lowest melting points are exhibited by which crystal system?


47. Which crystal system has unusually high vapour pressure?


48. Ice is and example of which crystal system?


49. Solid acetic acid is an example of which type of crystals?

A) Ionic B) Covalent C) Hydrogen bonded D) Polar Molecular

50. On increasing pressure, the boiling point of the substance?

A) Increases B) Decreases C) Remains Same D) It fluctuates

51. If 80 g of NaOH is dissolved in 2000g of water, what will be the freezing point of solution?

A) -0.51°C B) -1.86°C C) -3.72°C D) -6.58°C

52. 180 g of acetic acid is mixed with 3kg of water. What would be the boiling point of the

solution?

A) 100°C B) 101.53°C C) 101.02 D) 100.51°C

53. 900g of C6H12O6 are mixed 1 kg of water. What would be the expected freezing point of this

saturated solution?

A) 102.55°C B) -9.3°C C) 9.3°C D) -102.55°C

Q54. 3 moles of a substance is dissolved in 1 litre water. What would be the boiling point?

A) 100.51°C B) 102.04°C C) 101.53°C D) 102.55°C



5 | P a g e o u t o f | 5


Q55. The pressure on a system containing water is reduced. The melting point will be? A) Increased B) Decreased C) Remains Constant D) Can’t be told

Q56. If 10 g of ice melts, then the total quantity of heat absorbed is?

A) 10 calories B) 80 calories C) 800 calories D) 800 kilocalories

Q57. 1 kg of water was heated from 4°C to 14°C. The total usage of calories would be?

A) 10 calories B) 100 calories C) 100 kilocalories D) 10 kilocalories

Q58. When the excited liquid molecules leave the surface and go into vapour state, the average

kinetic energy of the molecules left at the surface becomes?

A) Higher B) Lower C) Remains Same D) Can’t be told

Q59. The surface tension of glycerol (C3H8O3) as compared to water is?

A) Higher B) Lower C) Same D) It varies

HYDROGEN AND WATER PREPARED BY


1 | P a g e o u t o f | 3


1. Which gas was an important fuel gas for homes and industry before the advent of natural gas

industry?

A) Methane Gas B) Water Gas C) Laughing Gas D) Producer Gas

2. The element that occurs most abundantly in compounds on earth is?

A) Carbon B) Oxygen C) Silicon D) Hydrogen

3. The most abundant, hydrogen containing compound is?

A) CH4 B) H2O C) HCl D) Both (A) and (B)

4. In an electrolytic process, how much electrical energy is required to produce 1 mole of H2?

A) 0.1 KWh B) 1 KWh C) 0.01 KWh D) 10 KWh

5. In the electrolysis of water, the volume of H2 gas produced is __________ to that of O2.

A) Equals B) One-half C) Twice D) One-fourth

6. Which celestial body has greater percentage of hydrogen atoms?

A) Earth B) Sun C) Moon D) Jupiter

7. Which of the following is not possible in case of Hydrogen?

A) Electronegativity B) 1st Ionization

Potential

C) Electron Affinity D) 2nd Ionization

Potential

8. Which of the following is much reactive?

A) Atomic Hydrogen B) Molecular

Hydrogen

C) Nascent Hydrogen D) Both (A) and (C)

9. Which hydrides are most stable against high temperatures?

A) Covalent Hydrides B) Complex Hydrides C) Ionic Hydrides D) Both (B) & (C)

10. Which hydride among covalent hydrides violates the general trend of low boiling point?

A) Hydrogen

monoxide

B) Hydrogen Chloride C) Hydrogen

Bromide

D) Hydrogen Iodide

11. The hydride that are non-stoichiometric in combination, are?

A) Ionic Hydrides B) Covalent Hydrides C) Metallic Hydrides D) Polymeric

Hydrides

12. Which Hydride(s) is/are non-conductors of electric current?

A) Ionic Hydrides B) Covalent Hydrides C) Metallic Hydrides D) Both (A) & (C)

13. The hydride that is the most appropriate source of nascent hydrogen, is?


Hydrides



2 | P a g e o u t o f | 3


14. Which of the following hydride is generally colourless? A) Ionic Hydrides B) Covalent Hydrides C) Polymeric

Hydrides

D) All (A), (B) & (C)

15. Which of the following hydride is generally not white in colour?


Hydrides

16. The Hydride family which comprised of the largest number of compounds, is?


Hydrides

17. Which hydrides are often used as catalysts?

A) Metallic Hydrides B) Complex Hydrides C) Polymeric

Hydrides

D) Both (A) & (B)

18. Which hydride among the following is an effective dehydrating agent?


Hydrides

19. The Hydride family has the least number of compounds, is?


Hydrides

20. Which hydrides are expected to be non-solids?


Hydrides

21. Which hydride group possess the magnetic properties?


Hydrides

22. The most important use of hydrides in industry is as?

A) Reducing agents B) Dehydrating Agent C) Source for Atomic

Hydrogen

D) Catalyst

23. Which hydrogen compound is used in the manufacture of fertilizers, plastics and explosives?

A) NH3 B) NaOH C) HCl D) None of the above

24. Hydrogen is used to convert benzene to cyclohexane, a cyclic hydrocarbon used as an

intermediate in the production of?

A) Fertilizers B) Plastics C) Explosives D) Nylon

25. Liquid Hydrogen is used a?

A) Bleaching Agent B) Reducing Agent C) Solvent D) Rocket Fuel



3 | P a g e o u t o f | 3


26. The rate of consumption of liquid hydrogen in space crafts is?

A) 3000 L/s B) 1.5 x 106 L/s C) 5.4 x 10

5 L/s D) 100 L/s

27. The oxyhydrogen torch is used to melt Tungsten. The minimum temperature of it’s flame is?

A) 3400°C B) 3000°C C) 1500°C D) 1000°C

28. Temporary hardness in water is observed due to the presence of?

A) HCO3- B) CO3

- C) Both (A) and (B) D) None

29. The precipitates of CaCO3, MgCO3, and FeCO3 are commonly called?

A) Boiler Scale B) Carbonate Ions C) Hard water residue D) Soft water residue

30. Temporary hard water is usually softened by addition of which base?

A) NaOH B) KOH C) Ca(OH)2 D) None

31. Permanent hard water is softened by which chemical compound?

A) Sulphur B) Baking Soda C) Washing Soda D) Alum

32. On softening of permanent hard water by Na2CO3, the remaining salts in solution are?

A) NaCl B) NaCO3 C) Na2SO4 D) Both (A) and (C)

33. The bond length of hydrogen bonds in water is about?

A) 180 pm B) 100 pm C) 150 pm D) 1 x 103 pm

34. The liquid water at 0°C is __________ dense than ice?

A) Less B) More C) Equally D) It varies

35. Sevaral compound such as CO, CO2, SO2, SO3 with higher molecular weight than water are

gases at room temperature, but water(mol. Wt= 18) is a liquid. This is primarily because of?

A) Polar Covalent

Bond

B) Laten Heat Values C) Hydrogen Bonding D) None

36. On freezing at O°C, the volume of water expands by about how many percent?

A) 9 % B) 20 % C) 200 % D) 50 %

37. In water cluster, a single water molecule is connected with _____ water molecules by H

bonds.

A) three B) four C) five D) six

38. Hydrogen is __________ soluble in water.

A) Slightly B) Readily C) Insoluble D) None

39. Hydrogen is __________ times heavier than air

A) 1/4 B) 1/24 C) 1/2 D) 1/14

ANSWER KEYS PREPARED BY

EXTRA MCQS HANDOUTS OSAMA HASAN



Answer Key for Extra MCQs Handout: Prepared by Osama Hasan


CHAPTER # 1

Topic: _______CHEMICAL BASICS________

1. A B C D E 38. A B C D E

2. A B C D E 39. A B C D E

3. A B C D E 40. A B C D E

4. A B C D E 41. A B C D E

5. A B C D E 42. A B C D E

6. A B C D E 43. A B C D E

7. A B C D E 44. A B C D E

8. A B C D E 45. A B C D E

9. A B C D E 46. A B C D E

10. A B C D E 47. A B C D E

11. A B C D E 48. A B C D E

12. A B C D E 49. A B C D E

13. A B C D E 50. A B C D E

14. A B C D E 51. A B C D E

15. A B C D E 52. A B C D E

16. A B C D E 53. A B C D E

17. A B C D E 54. A B C D E

18. A B C D E 55. A B C D E

19. A B C D E 56. A B C D E

20. A B C D E 57. A B C D E

21. A B C D E 58. A B C D E

22. A B C D E 59. A B C D E

23. A B C D E 60. A B C D E

24. A B C D E 61. A B C D E

25. A B C D E 62. A B C D E

26. A B C D E 63. A B C D E

27. A B C D E 64. A B C D E

28. A B C D E 65. A B C D E

29. A B C D E 66. A B C D E

30. A B C D E 67. A B C D E

31. A B C D E 68. A B C D E

32. A B C D E 69. A B C D E

33. A B C D E 70. A B C D E

34. A B C D E 71. A B C D E

35. A B C D E 72. A B C D E

36. A B C D E 73. A B C D E

37. A B C D E 74. A B C D E

CHAPTER # 2

Topic: _____CHEMICAL LANGUAGE____

1. A B C D E 38. A B C D E

2. A B C D E 39. A B C D E

3. A B C D E 40. A B C D E

4. A B C D E 41. A B C D E

5. A B C D E 42. A B C D E

6. A B C D E 43. A B C D E

7. A B C D E 44. A B C D E

8. A B C D E 45. A B C D E

9. A B C D E 46. A B C D E

10. A B C D E 47. A B C D E

11. A B C D E 48. A B C D E

12. A B C D E 49. A B C D E

13. A B C D E 50. A B C D E

14. A B C D E 51. A B C D E

15. A B C D E 52. A B C D E

16. A B C D E 53. A B C D E

17. A B C D E 54. A B C D E

18. A B C D E 55. A B C D E

19. A B C D E 56. A B C D E

20. A B C D E 57. A B C D E

21. A B C D E 58. A B C D E

22. A B C D E 59. A B C D E

23. A B C D E 60. A B C D E

24. A B C D E 61. A B C D E

25. A B C D E 62. A B C D E

26. A B C D E 63. A B C D E

27. A B C D E 64. A B C D E

28. A B C D E 65. A B C D E

29. A B C D E 66. A B C D E

30. A B C D E 67. A B C D E

31. A B C D E 68. A B C D E

32. A B C D E 69. A B C D E

33. A B C D E 70. A B C D E

34. A B C D E 71. A B C D E

35. A B C D E 72. A B C D E

36. A B C D E 73. A B C D E

37. A B C D E 74. A B C D E







CHAPTER # 3

Topic: ___CHEMICAL TECHNIQUES__

1. A B C D E 38. A B C D E

2. A B C D E 39. A B C D E

3. A B C D E 40. A B C D E

4. A B C D E 41. A B C D E

5. A B C D E 42. A B C D E

6. A B C D E 43. A B C D E

7. A B C D E 44. A B C D E

8. A B C D E 45. A B C D E

9. A B C D E 46. A B C D E

10. A B C D E 47. A B C D E

11. A B C D E 48. A B C D E

12. A B C D E 49. A B C D E

13. A B C D E 50. A B C D E

14. A B C D E 51. A B C D E

15. A B C D E 52. A B C D E

16. A B C D E 53. A B C D E

17. A B C D E 54. A B C D E

18. A B C D E 55. A B C D E

19. A B C D E 56. A B C D E

20. A B C D E 57. A B C D E

21. A B C D E 58. A B C D E

22. A B C D E 59. A B C D E

23. A B C D E 60. A B C D E

24. A B C D E 61. A B C D E

25. A B C D E 62. A B C D E

26. A B C D E 63. A B C D E

27. A B C D E 64. A B C D E

28. A B C D E 65. A B C D E

29. A B C D E 66. A B C D E

30. A B C D E 67. A B C D E

31. A B C D E 68. A B C D E

32. A B C D E 69. A B C D E

33. A B C D E 70. A B C D E

34. A B C D E 71. A B C D E

35. A B C D E 72. A B C D E

36. A B C D E 73. A B C D E

37. A B C D E 74. A B C D E

CHAPTER # 4

Topic: ________PERIODIC TABLE_______

1. A B C D E 38. A B C D E

2. A B C D E 39. A B C D E

3. A B C D E 40. A B C D E

4. A B C D E 41. A B C D E

5. A B C D E 42. A B C D E

6. A B C D E 43. A B C D E

7. A B C D E 44. A B C D E

8. A B C D E 45. A B C D E

9. A B C D E 46. A B C D E

10. A B C D E 47. A B C D E

11. A B C D E 48. A B C D E

12. A B C D E 49. A B C D E

13. A B C D E 50. A B C D E

14. A B C D E 51. A B C D E

15. A B C D E 52. A B C D E

16. A B C D E 53. A B C D E

17. A B C D E 54. A B C D E

18. A B C D E 55. A B C D E

19. A B C D E 56. A B C D E

20. A B C D E 57. A B C D E

21. A B C D E 58. A B C D E

22. A B C D E 59. A B C D E

23. A B C D E 60. A B C D E

24. A B C D E 61. A B C D E

25. A B C D E 62. A B C D E

26. A B C D E 63. A B C D E

27. A B C D E 64. A B C D E

28. A B C D E 65. A B C D E

29. A B C D E 66. A B C D E

30. A B C D E 67. A B C D E

31. A B C D E 68. A B C D E

32. A B C D E 69. A B C D E

33. A B C D E 70. A B C D E

34. A B C D E 71. A B C D E

35. A B C D E 72. A B C D E

36. A B C D E 73. A B C D E

37. A B C D E 74. A B C D E







CHAPTER # 5

Topic: ______STATES OF MATTER______

1. A B C D E 38. A B C D E

2. A B C D E 39. A B C D E

3. A B C D E 40. A B C D E

4. A B C D E 41. A B C D E

5. A B C D E 42. A B C D E

6. A B C D E 43. A B C D E

7. A B C D E 44. A B C D E

8. A B C D E 45. A B C D E

9. A B C D E 46. A B C D E

10. A B C D E 47. A B C D E

11. A B C D E 48. A B C D E

12. A B C D E 49. A B C D E

13. A B C D E 50. A B C D E

14. A B C D E 51. A B C D E

15. A B C D E 52. A B C D E

16. A B C D E 53. A B C D E

17. A B C D E 54. A B C D E

18. A B C D E 55. A B C D E

19. A B C D E 56. A B C D E

20. A B C D E 57. A B C D E

21. A B C D E 58. A B C D E

22. A B C D E 59. A B C D E

23. A B C D E 60. A B C D E

24. A B C D E 61. A B C D E

25. A B C D E 62. A B C D E

26. A B C D E 63. A B C D E

27. A B C D E 64. A B C D E

28. A B C D E 65. A B C D E

29. A B C D E 66. A B C D E

30. A B C D E 67. A B C D E

31. A B C D E 68. A B C D E

32. A B C D E 69. A B C D E

33. A B C D E 70. A B C D E

34. A B C D E 71. A B C D E

35. A B C D E 72. A B C D E

36. A B C D E 73. A B C D E

37. A B C D E 74. A B C D E

CHAPTER # 13

Topic: ___HYDROGEN AND WATER__

1. A B C D E 38. A B C D E

2. A B C D E 39. A B C D E

3. A B C D E 40. A B C D E

4. A B C D E 41. A B C D E

5. A B C D E 42. A B C D E

6. A B C D E 43. A B C D E

7. A B C D E 44. A B C D E

8. A B C D E 45. A B C D E

9. A B C D E 46. A B C D E

10. A B C D E 47. A B C D E

11. A B C D E 48. A B C D E

12. A B C D E 49. A B C D E

13. A B C D E 50. A B C D E

14. A B C D E 51. A B C D E

15. A B C D E 52. A B C D E

16. A B C D E 53. A B C D E

17. A B C D E 54. A B C D E

18. A B C D E 55. A B C D E

19. A B C D E 56. A B C D E

20. A B C D E 57. A B C D E

21. A B C D E 58. A B C D E

22. A B C D E 59. A B C D E

23. A B C D E 60. A B C D E

24. A B C D E 61. A B C D E

25. A B C D E 62. A B C D E

26. A B C D E 63. A B C D E

27. A B C D E 64. A B C D E

28. A B C D E 65. A B C D E

29. A B C D E 66. A B C D E

30. A B C D E 67. A B C D E

31. A B C D E 68. A B C D E

32. A B C D E 69. A B C D E

33. A B C D E 70. A B C D E

34. A B C D E 71. A B C D E

35. A B C D E 72. A B C D E

36. A B C D E 73. A B C D E

37. A B C D E 74. A B C D E


MCQS HANDOUT 5 OSAMA HASAN

NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,

KARACHI.

1

1. Intermolecular forces are the forces that exist between?

A) Atoms B) Molecules C) Ions D) All

2. The properties which mainly depend on the arrangement of atoms in a molecule are called?

A) Physical

Properties

B) Constitutive

Properties

C) Chemical

Properties

D) None

3. The properties which are the sum of the corresponding properties of individual components of

a system are known as?

A) Additive

Properties

B) Colligative

Properties

C) Chemical

Properties

D) None

4. Vander Walls forces are?

A) Permanent B) Temporary C) Elastic D) None

5. The KMT of gases gives an explanation to the __________ nature of gases.

A) Internal B) External C) Physical D) Chemical

6. The tiny particles that make up all the gases are called?

A) Ions & molecules B) Atoms& molecules C) Ions & Radicals D) Radical&molecules

7. In KMT of gases, a force among the molecules of gases is accepted which is?

A) Attractive B) Repulsive C) Gravitational D) Negligible

8. Which gas diffuses more rapidly?

A) O2 B) SO3 C) NH3 D) H2

9. A gas lesser in density than air can replace water by?

A) Downward

Delivery

B) Dissolving in

water

C) Upward Delivery D) Removing water

10. At the same temperature, the molecules of every gas have the same __________ energy.

A) Potential Energy B) Rotational Energy C) Vibrational Energy D) Kinetic Energy

11. The plot of ‘V’ against ‘1/P’ results in a?

A) Parabola B) Hyperbola C) Straight line D) Curve

12. The rate of diffusion of H2 and O2 is?

A) 1 : 4 B) 4 : 1 C) 1 : 8 D) 1 : 16

13. Glycerine decomposes at its?

A) Boiling Point B) Melting Point C) Critical Pont D) None

14. Which one of the following is the most strongly polar liquid?

A) Water B) Alcohol C) Hydrogen chloride D) Gasoline




KARACHI.

2

15. Which doesn’t affect the rate of evaporation?

A) Temperature B) Surface Area C) Intermolecular

Forces

D) Moles

16. Evaporation occurs at?

A) High Temperature B) Low Temperature C) All Temperatures D) None

17. The viscosity of H2O is more than CH3OH due to?

A) Covalent

Bonding

B) Ionic Bonding C) H - Bonding D) None

18. The tendency of a liquid to cling together is called?

A) Surface Tension B) Cohesion C) Adhesion D) Viscosity

19. Rain drops have spherical shape because a sphere has the least?

A) Area B) Volume C) Length D) Surface to Volume

Ration

20. Which liquid doesn’t wet glass?

A) Water B) Mercury C) Alcohol D) Ether

21. Latent Heat of Vaporization of water is?

A) 30 JK-1 mol

-1 B) 40 JK

-1 mol

-1 C) 40.7 JK

-1 mol

-1 D) 30.7 JK

-1 mol

-1

22. Which doesn’t affect the vapour pressure?

A) Nature of Liquid B) Intermolecular

Forces

C) Temperature D) Viscosity

23. Which is a covalent crystal?

A) I2 B) CO2 C) SiO2 D) KCl

24. The air we breathe in, is richer in oxygen content at?

A) Night B) Evening C) Noon D) Morning

25. Boiling Point of a solution is independent of?

A) Amount of

solution

B) Concentration C) Pressure D) Nature of solvent

26. According to KMT, kinetic energy of molecules increases when they are?

A) Mixed with mol. of

low temp.

B) Frozen in to solid C) Condensed into a

liquid

D) Melted from solid

to a liquid state.

27. Which of the following gases has the lowest density under room temperature?

A) CO B) NH3 C) N2 D) O2

28. The volume of a gas would theoretically be zero at?

A) 0 °C B) O K C) 273 K D) 273 °C




KARACHI.

3

29. 5 dm3 of a gas weights 12.5 g at S.T.P; Find its mass?

A) 50 g/mol B) 12.5 g/mol C) 62.5 g/mol D) 56 g/mol

30. The breaking system of a car contains liquid. The reason for using a liquid because it?

A) Cannot be

compressed

B) Readily turns to a

gas

C) Takes up the

shape of

container

D) Distributes pressure

in all directions

uniformly

31. Microscopic view of two liquids is:

Which one is expected to be more viscous?

A) II B) I C) Both have same

viscosity

D) Couldn’t be

predicted.

32. The viscosity of water is?

A) More than ether B) Less than ether C) Equal to ether D) It varies

33. Viscosity of a substance decreases with?

A) Increase in

intermolecular

forces

B) Increase in

temperature

C) Decrease in

temperature

D) Decrease in mol.

Wt. of substance

34. The boiling point of water at 100 torr will be?

A) 100 °C B) Higher than 100 °C C) Lower than 100°C D) 0 °C

35. The gas that’ll liquefy most differently would be?

A) CO2 B) H0 C) He D) NH3

36. Solid Iodine crystal is a type of?

A) Covalent Crystal B) Ionic Crystal C) Metallic Crystal D) Molecular Crystal

37. The property of a substance which depends on the arrangement of atoms is?

A) Colligative B) Constitutive C) Additive D) Anisotropic

38. Covalent crystal like diamond....?

A) Have high

melting point

B) Low density C) High refractive

index

D) All of these

39. Which one of the following is an amorphous form of carbon?

A) Graphite B) Charcoal C) 14C isotope D) All of these




KARACHI.

4

A�SWER KEY

1. A B C D E 38. A B C D E

2. A B C D E 39. A B C D E

3. A B C D E 40. A B C D E

4. A B C D E 41. A B C D E

5. A B C D E 42. A B C D E

6. A B C D E 43. A B C D E

7. A B C D E 44. A B C D E

8. A B C D E 45. A B C D E

9. A B C D E 46. A B C D E

10. A B C D E 47. A B C D E

11. A B C D E 48. A B C D E

12. A B C D E 49. A B C D E

13. A B C D E 50. A B C D E

14. A B C D E 51. A B C D E

15. A B C D E 52. A B C D E

16. A B C D E 53. A B C D E

17. A B C D E 54. A B C D E

18. A B C D E 55. A B C D E

19. A B C D E 56. A B C D E

20. A B C D E 57. A B C D E

21. A B C D E 58. A B C D E

22. A B C D E 59. A B C D E

23. A B C D E 60. A B C D E

24. A B C D E 61. A B C D E

25. A B C D E 62. A B C D E

26. A B C D E 63. A B C D E

27. A B C D E 64. A B C D E

28. A B C D E 65. A B C D E

29. A B C D E 66. A B C D E

30. A B C D E 67. A B C D E

31. A B C D E 68. A B C D E

32. A B C D E 69. A B C D E

33. A B C D E 70. A B C D E

34. A B C D E 71. A B C D E

35. A B C D E 72. A B C D E

36. A B C D E 73. A B C D E

37. A B C D E 74. A B C D E

chemistry mcqs handouts

Documents