Class 11 Chemistry Chapter 4 – Stoichiometry MCQs | FBISE | Grade 11 Chemistry

Description: Practice 50 exam-oriented MCQs from Class 11 Chemistry Chapter 4 – Stoichiometry, covering relative atomic and molecular masses, mole concept, Avogadro’s number, molar mass, empirical and molecular formulae, chemical equations, limiting reactants, and percentage yield.

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1. Stoichiometry is the quantitative study of

A) chemical reactions and their reactants and products
B) atomic nuclei only
C) chemical colours only
D) laboratory apparatus

2. The SI unit of amount of substance is the

A) gram
B) mole
C) litre
D) kilogram

3. One mole of a substance contains approximately

A) 3.011 × 10^23 particles
B) 6.022 × 10^22 particles
C) 6.022 × 10^23 particles
D) 1.000 × 10^23 particles

4. The number 6.022 × 10^23 is known as

A) Planck constant
B) Faraday constant
C) gas constant
D) Avogadro’s number

5. The mass of one mole of a substance is its

A) molar mass
B) atomic number
C) density
D) molecular volume

6. The molar mass of carbon-12 is defined as

A) 6 g mol−1
B) 12 g mol−1
C) 12 kg mol−1
D) 24 g mol−1

7. The relative atomic mass of an element is a comparison with

A) one mole of oxygen
B) one gram of hydrogen
C) one-twelfth of the mass of a carbon-12 atom
D) the mass of an electron

8. The relative molecular mass of a compound is the sum of the

A) molar volumes
B) atomic numbers only
C) neutron numbers only
D) relative atomic masses of its atoms

9. The formula mass is commonly used for

A) ionic compounds
B) only gases
C) only organic molecules
D) only elements

10. The number of moles in a sample is calculated by dividing its mass by its

A) density
B) molar mass
C) volume
D) atomic number

11. The formula for number of moles from mass is

A) n = mM
B) n = M/m
C) n = m/M
D) n = m + M

12. The molar mass of H2O is approximately

A) 10 g mol−1
B) 16 g mol−1
C) 20 g mol−1
D) 18 g mol−1

13. One mole of H2O contains

A) 6.022 × 10^23 water molecules
B) 3.011 × 10^23 water molecules
C) 18 water molecules
D) 1.0 × 10^23 oxygen atoms only

14. One mole of sodium ions contains

A) 6.022 × 10^23 electrons only
B) 6.022 × 10^23 Na+ ions
C) 23 Na+ ions
D) 1.0 × 10^23 ions

15. The number of particles in a given amount of substance is related to

A) pressure only
B) density only
C) moles and Avogadro’s number
D) atomic radius only

16. A balanced chemical equation obeys the law of

A) conservation of density
B) conservation of volume only
C) conservation of temperature
D) conservation of mass

17. Coefficients in a balanced chemical equation represent

A) mole ratios
B) atomic masses
C) densities
D) melting points

18. The equation 2H2 + O2 → 2H2O shows that hydrogen and oxygen react in a mole ratio of

A) 1:1
B) 2:1
C) 1:2
D) 2:2

19. The simplest whole-number ratio of atoms in a compound is its

A) structural formula
B) molecular formula
C) empirical formula
D) ionic charge

20. The molecular formula shows the

A) number of isotopes
B) simplest ratio only
C) number of neutrons
D) actual number of atoms of each element in a molecule

21. An empirical formula can be converted into a molecular formula using the

A) molar mass
B) boiling point only
C) density of water only
D) atomic number only

22. The empirical formula of glucose, C6H12O6, is

A) C6H12O6
B) CH2O
C) CHO
D) C2H4O2

23. The molecular formula of a compound is an integer multiple of its

A) molar volume
B) atomic number
C) empirical formula
D) ionic charge

24. Percentage composition gives the percentage by mass of each

A) ion in a solution
B) neutron in an atom
C) molecule in a gas
D) element in a compound

25. The percentage by mass of an element is calculated from its mass contribution divided by the

A) molar mass of the compound
B) atomic number
C) number of neutrons
D) gas volume

26. A limiting reactant is the reactant that

A) is always present in excess
B) is consumed first and limits product formation
C) has the greatest molar mass
D) is never consumed

27. The reactant left over after a reaction is complete is called the

A) product
B) limiting reactant
C) excess reactant
D) catalyst

28. The amount of product predicted from the limiting reactant is the

A) excess yield
B) actual yield
C) percentage yield
D) theoretical yield

29. The amount of product actually obtained in an experiment is the

A) actual yield
B) theoretical yield
C) molar yield
D) limiting yield

30. Percentage yield is calculated as

A) theoretical yield ÷ actual yield × 100
B) actual yield ÷ theoretical yield × 100
C) actual yield + theoretical yield
D) theoretical yield − actual yield

31. If actual yield equals theoretical yield, the percentage yield is

A) 0%
B) 50%
C) 100%
D) 200%

32. A chemical equation provides information about the relative

A) melting points
B) colours of substances
C) densities of all substances
D) amounts of reactants and products

33. The coefficients of a balanced equation can be used to establish

A) stoichiometric mole ratios
B) atomic radii
C) electronegativity values
D) bond angles

34. For the reaction N2 + 3H2 → 2NH3, one mole of N2 reacts with

A) 2 moles of H2
B) 3 moles of H2
C) 1 mole of H2
D) 6 moles of H2

35. For N2 + 3H2 → 2NH3, two moles of NH3 require

A) 3 moles of N2
B) 2 moles of N2
C) 1 mole of N2
D) 6 moles of N2

36. If 2 moles of H2 react completely according to 2H2 + O2 → 2H2O, the amount of H2O formed is

A) 0.5 mole
B) 1 mole
C) 4 moles
D) 2 moles

37. The theoretical amount of product is determined using the

A) balanced chemical equation
B) unbalanced equation
C) colour of reactants
D) reaction vessel size only

38. A mole ratio is obtained from the

A) subscripts alone
B) coefficients of a balanced equation
C) atomic symbols alone
D) physical states only

39. The reagent that determines the maximum amount of product formed is the

A) catalyst
B) solvent
C) limiting reactant
D) excess product

40. If a reactant is present in a quantity greater than required by the balanced equation, it is

A) a product
B) limiting
C) a catalyst
D) in excess

41. A balanced equation for a reaction between calcium and oxygen is

A) 2Ca + O2 → 2CaO
B) Ca + O2 → CaO2
C) Ca2 + O → Ca2O
D) Ca + 2O2 → CaO

42. The coefficient of oxygen in 2H2 + O2 → 2H2O is

A) 2
B) 1
C) 3
D) 4

43. The coefficient of ammonia in N2 + 3H2 → 2NH3 is

A) 3
B) 1
C) 2
D) 6

44. The formula mass of NaCl is approximately

A) 18 u
B) 35.5 u
C) 23 u
D) 58.5 u

45. The molar mass of CO2 is approximately

A) 44 g mol−1
B) 28 g mol−1
C) 32 g mol−1
D) 18 g mol−1

46. The number of moles in 44 g of CO2 is

A) 2 mol
B) 1 mol
C) 0.5 mol
D) 44 mol

47. The number of moles in 18 g of H2O is approximately

A) 0.5 mol
B) 2 mol
C) 1 mol
D) 18 mol

48. One mole of oxygen gas, O2, contains

A) 2 × 6.022 × 10^23 oxygen atoms only
B) 3.011 × 10^23 O2 molecules
C) 16 O2 molecules
D) 6.022 × 10^23 O2 molecules

49. Two moles of oxygen gas contain

A) 2 × 6.022 × 10^23 O2 molecules
B) 6.022 × 10^23 O2 molecules
C) 3.011 × 10^23 O2 molecules
D) 2 O2 molecules

50. Stoichiometric calculations are most reliable when the chemical equation is

A) unbalanced
B) correctly balanced
C) written without formulas
D) based only on physical appearance

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Class 11 Chemistry Chapters

Syllabus & SLO Alignment

This chapter follows the FBISE HSSC-I Chemistry Assessment Framework based on the National Curriculum of Pakistan 2022–23. The relevant SLO range for this chapter is C-11-B-50 to C-11-B-59. The SLOs cover the chapter content and include the learning outcomes identified by FBISE for this content area. Summative/formative status follows the official assessment framework.

Class 11 Chemistry Chapter 4 – Stoichiometry MCQs | FBISE | Grade 11 Chemistry

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Class 11 Chemistry Chapters

Syllabus & SLO Alignment

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