MDCAT XI Chemistry Stoichiometry Online Test 2026

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Created on January 19, 2026 By

old.medicoengineer.com

MDCAT XI Chemistry Stoichiometry Online Test 2026

📚 Test Details

Subject: Chemistry
Class: 1st year / XI
Chapter: Stoichiometry
Test: 3
Book: Sindh Textbook
Total No. Of MCQs: 50 MCQs
Time Allowed: 50 Minutes
Price: Free

NameEmailPhone Number

1 / 50

1. Q.1 One mole of Na⁺ ions contains the same number of particles as:

a) 1 mole of Na atoms

b) 0.5 mole of Na₂ molecules

c) 1 mole of Cl⁻ ions

d) 1 gram of Na

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2. Q.2 The number of moles of electrons in 1 mole of Mg²⁺ ions is:

a) 10

b) 12

c) 24

d) 2

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3. Q.3 Avogadro’s number is most directly used to convert between:

a) Mass and volume

b) Moles and particles

c) Pressure and volume

d) Density and mass

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4. Q.4 A compound contains 40% C, 6.67% H and 53.33% O. Its empirical formula is:

a) CH₂O

b) C₂H₄O₂

c) C₃H₆O₃

d) CH₄O

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5. Q.5 If molecular mass equals empirical formula mass, then the compound:

a) Must be ionic

b) Has same molecular and empirical formula

c) Cannot exist

d) Is always gaseous

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6. Q.6 Which percentage composition gives empirical formula NH₃?

a) N = 14%, H = 86%

b) N = 82.35%, H = 17.65%

c) N = 70%, H = 30%

d) N = 50%, H = 50%

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7. Q.7 Which statement is correct?

a) Empirical formula shows actual number of atoms

b) Molecular formula is simplest ratio

c) Empirical formula gives simplest whole-number ratio

d) Molecular and empirical formulas are always same

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8. Q.8 Which compound has same empirical and molecular formula?

a) C₂H₄

b) C₆H₆

c) H₂O

d) C₄H₈

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9. Q.9 In a balanced equation, coefficients represent:

a) Mass ratio

b) Volume ratio

c) Mole ratio

d) Density ratio

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10. Q.10 How many grams of CO₂ are produced when 11 g C reacts completely?

a) 22 g

b) 33 g

c) 44 g

d) 11 g

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11. Q.11 Which reactant determines theoretical yield?

a) Excess reactant

b) Catalyst

c) Limiting reactant

d) Product

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12. Q.12 How many moles of NaCl are formed from 1 mole of Na₂CO₃?

a) 1

b) 2

c) 0.5

d) Depends on pressure

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13. Q.13 If actual yield equals theoretical yield, percent yield is:

a) 0%

b) 50%

c) 100%

d) Undefined

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14. Q.14 Which factor does not affect percent yield?

a) Side reactions

b) Purity of reactants

c) Temperature

d) Balanced equation coefficients

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15. Q.15 Which situation gives maximum yield?

a) Limiting reactant in large amount

b) No limiting reactant

c) Perfect stoichiometric ratio

d) Excess product

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16. Q.16 If 80 g product is obtained instead of 100 g theoretical, percent yield is:

a) 20%

b) 80%

c) 100%

d) 125%

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17. Q.17 If a reactant is in excess, then:

a) Reaction rate increases

b) Theoretical yield increases

c) Some reactant remains unreacted

d) Percent yield decreases necessarily

18 / 50

18. Q.18 Which is always true?

a) Actual yield ≥ theoretical yield

b) Actual yield ≤ theoretical yield

c) Percent yield > 100

d) Yield is independent of reaction conditions

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19. Q.19 Limiting reagent is identified by comparing:

a) Masses only

b) Volumes only

c) Mole ratios

d) Densities

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20. Q.20 At same temperature and pressure, mole ratio of gases equals:

a) Mass ratio

b) Density ratio

c) Volume ratio

d) Pressure ratio

21 / 50

21. Q.21 Which gas will occupy maximum volume at STP for same mass?

a) CO₂

b) O₂

c) H₂

d) N₂

22 / 50

22. Q.22 Which condition is necessary for volume–volume relationship in reactions?

a) Same mass

b) Same pressure & temperature

c) Same density

d) Same molecular mass

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23. Q.23 Which law is most directly applied in gaseous stoichiometry?

a) Boyle’s law

b) Charles’ law

c) Avogadro’s law

d) Dalton’s law

24 / 50

24. Q.24 Which gas law explains mole–volume relationship?

a) Boyle

b) Charles

c) Avogadro

d) Graham

25 / 50

25. Q.25 Which reaction best illustrates law of combining volumes?

a) Na + Cl → NaCl

b) H₂ + O₂ → H₂O

c) AgNO₃ + NaCl → AgCl

d) CaCO₃ → CaO + CO₂

26 / 50

26. Q.26 Volume ratios in gaseous reactions are always:

a) Fractional

b) Whole numbers

c) Irrational

d) Random

27 / 50

27. Q.27 The formula for percentage yield is:

a) (Theoretical yield / Actual yield) × 100

b) (Actual yield / Theoretical yield) × 100

c) (Limiting reactant / Excess reactant) × 100

d) (Product / Reactant) × 100

28 / 50

28. Q.28 If theoretical yield doubles while actual yield remains constant, percentage yield will:

a) Double

b) Remain same

c) Become half

d) Become zero

29 / 50

29. Q.29 Which law explains balancing of chemical equations?

a) Definite proportions

b) Multiple proportions

c) Conservation of mass

d) Combining volumes

30 / 50

30. Q.30 Which concentration unit is temperature independent?

a) Molarity

b) Normality

c) Molality

d) Volume %

31 / 50

31. Q.31 Which pair has the same number of moles?

a) 22 g CO₂ and 16 g O₂

b) 28 g N₂ and 32 g O₂

c) 1 g H₂ and 16 g O₂

d) 12 g C and 32 g O₂

32 / 50

32. Q.32 Methane reacts with steam: CH₄ + H₂O → CO + 3H₂. Limiting reactant?

a) CH₄

b) H₂O

c) CO

33 / 50

33. Q.33 Actual yield = 380 g, theoretical yield = 500 g. Percentage yield?

a) 90%

b) 98%

c) 76%

d) 132%

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34. Q.34 In a vessel, 20 g He, 20 g F₂, 20 g Cl₂ are present. Least atoms?

a) He

b) F₂

c) Cl₂

d) He & F₂

35 / 50

35. Q.35 Total number of covalent bonds in 9 g of water is:

a) 6.02 × 10²³

b) 6.02 × 10²²

c) 3.01 × 10²³

d) 3.01 × 10²²

36 / 50

36. Q.36 Hydrocarbon molar mass 72 g/mol, 83.3% carbon. Molecular formula?

a) C₆H₁₂

b) C₅H₁₂

c) C₅H₁₀

d) C₆H₁₀

37 / 50

37. Q.37 In industrial chemical reactions, percent yield is usually:

a) 100%

b) <100%

c) >100%

d) Zero

38 / 50

38. Q.38 If reactants are in excess, actual yield is always:

a) Equal to theoretical yield

b) Less than or equal to theoretical yield

c) Greater than theoretical yield

d) Zero

39 / 50

39. Q.39 Which statement is true?

a) Limiting reagent is always the reactant in smaller mass

b) Limiting reagent is the reactant present in smallest number of moles considering stoichiometry

c) Limiting reagent has the smallest molar mass

d) Limiting reagent can be identified by density

40 / 50

40. Q.40 For N₂ + 3H₂ → 2NH₃, identify H₂ as limiting reactant:

a) 14 g N₂ + 4 g H₂

b) 3 g N₂ + 8 g H₂

c) 28 g N₂ + 6 g H₂

d) 56 g N₂ + 10 g H₂

41 / 50

41. Q.41 Which term is used for 18 g H₂O?

a) g-atom

b) g-ions

c) g-formula unit

d) g-molecule

42 / 50

42. Q.42 Total number of atoms in 192 g of SO₂ gas?

a) 4Nₐ

b) 5Nₐ

c) 6Nₐ

d) 9Nₐ

43 / 50

43. Q.43 In 2Al + 3Cl₂ → 2AlCl₃, 10 g Al reacts with 20 g Cl₂. Limiting reagent?

a) Al

b) Cl₂

c) Both

d) None

44 / 50

44. Q.44 Percent yield = 75%, theoretical yield = 20 g. Actual product?

a) 15 g

b) 25 g

c) 10 g

d) 20 g

45 / 50

45. Q.45 Side reactions lower:

a) Actual yield

b) % yield

c) Both A & B

d) Neither

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46. Q.46 Which statement is correct?

a) Stoichiometry relates mass and number of particles in a chemical reaction

b) Stoichiometry only applies to gases

c) Stoichiometry ignores limiting reagents

d) Stoichiometry does not depend on balanced equations

47 / 50

47. Q.47 A limiting reagent:

a) Is always the reactant present in smaller mass

b) Is completely consumed first in a chemical reaction

c) Remains in excess after reaction

d) Does not affect the amount of product formed

48 / 50

48. Q.48 The theoretical yield of a reaction:

a) Is always equal to actual yield

b) Depends on limiting reagent

c) Depends on excess reagent

d) Is independent of stoichiometry

49 / 50

49. Q.49 Percent yield can be greater than 100% because:

a) More reactant was added

b) Impurities are present in the product

c) Limiting reagent increased

d) Reaction occurs in gas phase

50 / 50

50. Q.50 Which compound has the same empirical formula as glucose (C₆H₁₂O₆)?

a) Ethanol

b) Acetic acid

c) Formaldehyde

d) Lactic acid

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MDCAT XI Chemistry Stoichiometry Online Test 2026

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