MDCAT XI Chemistry Stoichiometry Online Test-2

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Created on June 12, 2025 By

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MDCAT XI Chemistry Stoichiometry Online Test-2

📚 Test Details

Subject: Chemistry
Class: 1st year / XI
Chapter Name: Stoichiometry
Test: 2
Book: Sindh Textbook
Total No. Of MCQs: 50 MCQs
Time Allowed: 50 Minutes
Price: Free

NameEmailPhone Number

1 / 50

1. According to the S.I. system, ___ is used to measure the amount of substance.

a) mole

b) weight machine

c) weight

d) mass

2 / 50

2. The number of particles or substances present in moles is known by:

a) Boltzmann constant

b) Avogadro’s number

c) Universal gas constant

d) Reynolds number

3 / 50

3. Azhar has 1 mole of N₂, which contains X number of particles, and Aamir has 1 mole of NH₃ (Note: NH₃ has twice the number of atoms than N₂). What is the number of particles in NH₃?

a) 2X

b) 3X

c) X

d) 4X

4 / 50

4. What will be the estimated practical yield of CO₂ obtained from 3 moles of carbon and 5 moles of oxygen gas?

a) 132 g

b) 220 g

c) 120 g

d) 136 g

5 / 50

5. Two molecules of same molar mass having the same given mass must have:
I. Same number of atoms
II. Same number of particles
III. Same number of moles

a) I, II, III

b) II, III

c) I, III

d) III

6 / 50

6. Find the incorrect statement about stoichiometry:

a) Greek word

b) Utilizes balanced chemical equation

c) Qualitative relation of reactants and products

d) All are correct

7 / 50

7. Ali loves ionic compounds, so he took 58.45 g of NaCl. Choose the best option:

a) He has 2 moles of NaCl

b) He has 6.02 × 10²³ Cl atoms

c) He has 12.06 × 10²³ Na atoms

d) None of these

8 / 50

8. 12.06 × 10²³ atoms of oxygen contain:

a) 2 moles of oxygen gas

b) 3 moles of oxygen gas

c) 1 mole of oxygen gas

d) 0.5 mole of oxygen gas

9 / 50

9. If 1 mole of alkyne combusts and produces 4 moles of CO₂, what is the hydrocarbon and how many moles of H₂O are produced?

a) Propyne, 4

b) Propyne, 3

c) Butyne, 4

d) Butyne, 3

10 / 50

10. What is the number of particles in 10 moles of hydrochloric acid?

a) 602.2 × 10²² particles

b) 6.022 × 10²³ particles

c) 6.22 × 10²³ particles

d) 3.22 × 10²² particles

11 / 50

11. During an experiment, 12.04 × 10²³ particles of CaCO₃ produced 40 g of CaO. What will be the percentage yield?

a) 71.42%

b) 35.71%

c) 68%

d) 48%

12 / 50

12. In a vessel, 20 g He, 20 g F₂, and 20 g Cl₂ are present. Which one will have the least number of atoms?

a) He

b) F₂

c) Cl₂

d) He & F₂

13 / 50

13. Consider the reaction:
2Na(s) + 2H₂O(l) ⟶ 2NaOH + H₂
When 69 g of Na reacts with water, the volume of H₂ gas obtained at room temperature is:

a) 33.6 L

b) 36 L

c) 33 L

d) 35.5 L

14 / 50

14. The volume occupied by 1.6 g of O₂ at STP is:

a) 2.24 dm³

b) 22.4 dm³

c) 1.12 dm³

d) 112 dm³

15 / 50

15. The total number of covalent bonds in 18 g of water (N_A is Avogadro's number) is:

a) N_A

b) 1.5 N_A

c) 2 N_A

d) 0.5 N_A

16 / 50

16. For the reaction 2A + B ⟶ C, the amount of C formed by starting the reaction with 5 moles of B and 8 moles of A is:

a) 5 moles

b) 8 moles

c) 16 moles

d) 4 moles

17 / 50

17. 1 dm³ of water contains how many moles?

a) 100

b) 1000

c) 50

d) 55.5

18 / 50

18. Which one of the following compounds contains the highest percentage by mass of nitrogen?

a) NH₃

b) NH₄OH

c) N₂H₄

d) NO

19 / 50

19. Number of moles of CO₂ that contain 16 g of oxygen is:

a) 0.25

b) 0.125

c) 0.50

d) 0.150

20 / 50

20. Number of hydrogen atoms in 6.0 g of acetic acid is:

a) 0.1 N_A

b) 0.2 N_A

c) 0.3 N_A

d) 0.4 N_A

21 / 50

21. In a particular reaction, one of the reactants limits the number of products formed. This is called the:

a) Limiting reagent

b) Limiting product

c) Excessive reagent

d) Excessive reactant

22 / 50

22. 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 sides

d) Follows the law of conservation of mass

23 / 50

23. 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

24 / 50

24. What is the amount of water produced when 8 g of hydrogen reacts with 32 g of oxygen?

a) 2 moles

b) 1 mole

c) 3 moles

d) 0.5 mole

25 / 50

25. Calculate the mass percent of magnesium in the formation of magnesium oxide.

a) 0.3

b) 1.5

c) 0.67

d) 0.6

26 / 50

26. In a container, there are 4 moles of nitrogen, 3 moles of oxygen, and 7 moles of hydrogen. Find the mole fraction of oxygen.

a) 0.2143

b) 0.2142

c) 0.1234

d) 0.2434

27 / 50

27. Find the amount of carbon dioxide produced by the combustion of 20 g of methane.

a) 44 g

b) 20 g

c) 55 g

d) 22 g

28 / 50

28. What is the balanced equation for:
CO₂ + H₂O → C₆H₁₂O₆ + O₂?

a) CO₂ + H₂O → C₆H₁₂O₆ + O₂

b) 6CO₂ + 6H₂O → C₆H₁₂O₆ + 6O₂

c) 6CO₂ + 6H₂O → C₆H₁₂O₆ + 2O₂

d) 3CO₂ + 2H₂O → C₆H₁₂O₆ + O₂

29 / 50

29. How many moles of CH₄ are required to produce 10 moles of H₂O in a combustion reaction (considering O₂ in excess)?

a) 1

b) 2

c) 5

d) 10

30 / 50

30. CH₄ + 2O₂ → CO₂ + 2H₂O
24 grams of CH₄ was added to the above reaction. Calculate the theoretical yield of CO₂.

a) 66 g

b) 132 g

c) 33 g

d) 8.72 g

31 / 50

31. Calculate the volume of CO₂ at STP that can be obtained by complete burning of 100 dm³ of butane:
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O

a) 200 dm³

b) 800 dm³

c) 400 dm³

d) 100 dm³

32 / 50

32. The number of moles in 6.4 g of SO₂:

a) 0.4

b) 2

c) 0.2

d) 0.1

33 / 50

33. Maximum number of molecules is present in:

a) 100 g H₂

b) 100 g N₂

c) 100 g CO₂

d) 100 g SO₂

34 / 50

34. Generally, actual yield is:

a) Greater than theoretical yield

b) Less than theoretical yield

c) Equal to the theoretical yield

d) Sometimes greater and sometimes less than theoretical yield

35 / 50

35. The volume of N₂ gas occupied by 1.5 moles at STP:

a) 22.4 dm³

b) 11.2 dm³

c) 44.8 dm³

d) 33.6 dm³

36 / 50

36. Molar mass of FeCl₃ is:

a) 170.25

b) 162.35

c) 156.35

d) 156.25

37 / 50

37. Mass-volume relationship is based on:

a) Law of Conservation of Mass

b) Gay-Lussac's Law

c) Avogadro’s Law

d) None of these

38 / 50

38. Which is the excess reactant in the reaction:
C₅H₁₂ + 8O₂ → 5CO₂ + 6H₂O, if the initial moles of C₅H₁₂ and O₂ are 2 and 8, respectively?

a) C₅H₁₂

b) O₂

c) CO₂

d) H₂O

39 / 50

39. Which is the limiting reactant in the reaction below?

C₅H₁₂ + 8O₂ → 5CO₂ + 6H₂O, if the initial moles of C₅H₁₂ and O₂ are 2 and 8, respectively?

a) C₅H₁₂

b) O₂

c) CO₂

d) H₂O

40 / 50

40. How many moles of C₅H₁₂ remain unreacted after completion?
C₅H₁₂ + 8O₂ → 5CO₂ + 6H₂O, if the initial moles of C₅H₁₂ and O₂ are 2 and 8, respectively?

a) 0

b) 1

c) 2

d) 3

41 / 50

41. One mole of any substance contains:

a) 6.022 × 10²⁶ particles

b) 6.022 × 10²² particles

c) 6.022 × 10²³ particles

d) 3.022 × 10²² particles

42 / 50

42. One mole of sucrose contains how many grams?

a) 342 g

b) 343 g

c) 341 g

d) 340 g

43 / 50

43. If 1 mole of ammonia is 17 g, then the mass of 0.3 moles is:

a) 21 g

b) 5.1 g

c) 17 g

d) 1 g

44 / 50

44. One mole of ethanol and one mole of ethane have an equal:

a) Mass

b) Number of atoms

c) Number of electrons

d) Number of molecules

45 / 50

45. Methane reacts with steam to form H₂ and CO:
CH₄ + H₂O → CO + 3H₂
What volume of H₂ can be obtained from 100 cm³ of methane at STP?

a) 300 cm³

b) 200 cm³

c) 150 cm³

d) 100 cm³

46 / 50

46. A flask contains 500 cm³ of SO₂ at STP. The flask contains:

a) 40 g

b) 100 g

c) 50 g

d) 1.427 g

47 / 50

47. What is the mass of aluminium in 204 g of aluminium oxide (Al₂O₃)?

a) 26 g

b) 27 g

c) 54 g

d) 108 g

48 / 50

48. The Avogadro's constant is the number of:

a) Atoms in 12 g of carbon-12

b) Molecules in 1 mole of a substance

c) Electrons in 1 g of hydrogen

d) Protons in 1 mole of a substance

49 / 50

49. If four moles of SO₂ are oxidized to SO₃, how many moles of O₂ are required?
2SO₂ + O₂ → 2SO₃

a) 0.5

b) 1.0

c) 1.5

d) 2.0

50 / 50

50. A ring was found to have 24 g of diamond. What is the number of atoms in it?

a) N_A

b) 2 N_A

c) 4 N_A

d) 3 N_A

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MDCAT XI Chemistry Stoichiometry Online Test-2

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