Skip to content
QuizQuip
Sign up
Back to Topic 3
Mark schemePDF

Topic 3 Practice Paper: Stoichiometry — question paper

QuizQuipPractice Series
QQ/IGCSE-CHEM/T3

IGCSE · Cambridge IGCSE Chemistry (Extended (Core + Supplement))

Topic 3 Practice Paper

Stoichiometry

Duration: 40 minutes
Total: 30 marks
Name:
Class:
Register No.:
Date:

READ THESE INSTRUCTIONS FIRST

  • Answer all questions.
  • Section A contains ten multiple-choice questions worth 10 marks. Choose one answer, A, B, C or D, for each.
  • Section B contains four structured questions worth 20 marks. Write your answers in the spaces provided.
  • The number of marks is given in brackets [ ] at the end of each question or part question.
  • The total mark for this paper is 30.

Original practice material written against the Cambridge IGCSE Chemistry syllabus. It is not an official Cambridge examination paper. Topic 3: Stoichiometry.

For Examiner’s Use
Section A/ 10
Section B/ 20
Total/ 30

Section A: Multiple-choice questions[10 marks]

Choose one answer for each question. Each question is worth 1 mark.

  1. 1

    What is the relative formula mass of sodium chloride, NaCl? (Aᵣ: Na = 23, Cl = 35.5)

    1. A58.5
    2. B35.5
    3. C23.0
    4. D81.0
    ( )
  2. 2

    Which formula is correct for aluminium oxide?

    1. AAlO
    2. BAl₂O₃
    3. CAl₃O₂
    4. DAl₂O
    ( )
  3. 3

    How many moles are there in 20 g of calcium carbonate, CaCO₃? (Mᵣ = 100)

    1. A0.10 mol
    2. B0.20 mol
    3. C0.50 mol
    4. D5.0 mol
    ( )
  4. 4

    What volume does 3.0 mol of any gas occupy at room temperature and pressure? (molar gas volume = 24 dm³)

    1. A24 dm³
    2. B48 dm³
    3. C60 dm³
    4. D72 dm³
    ( )
  5. 5

    0.50 mol of a solute is dissolved to make 2.0 dm³ of solution. What is the concentration?

    1. A2.0 mol/dm³
    2. B1.0 mol/dm³
    3. C0.25 mol/dm³
    4. D0.40 mol/dm³
    ( )
  6. 6

    What is the percentage by mass of nitrogen in ammonia, NH₃? (Aᵣ: N = 14, H = 1)

    1. A17%
    2. B47%
    3. C50%
    4. D82%
    ( )
  7. 7

    Glucose has the molecular formula C₆H₁₂O₆. What is its empirical formula?

    1. ACH₂O
    2. BC₆H₁₂O₆
    3. CC₃H₆O₃
    4. DCHO
    ( )
  8. 8

    What is the mass of 0.50 mol of water? (Mᵣ = 18)

    1. A36 g
    2. B18 g
    3. C9.0 g
    4. D2.0 g
    ( )
  9. 9

    In the reaction N₂ + 3H₂ → 2NH₃, 28 g of nitrogen reacts with 6 g of hydrogen to give 34 g of ammonia. What mass of ammonia forms from 14 g of nitrogen?

    1. A17 g
    2. B14 g
    3. C34 g
    4. D8.5 g
    ( )
  10. 10

    Which equation is the correct ionic equation for the neutralisation of an acid by an alkali?

    1. ANa⁺ + Cl⁻ → NaCl
    2. B2H⁺ + 2OH⁻ → 2H₂O
    3. CH⁺ + Cl⁻ → HCl
    4. DH⁺ + OH⁻ → H₂O
    ( )

Section B: Structured questions[20 marks]

Answer all questions in the spaces provided.

  1. 11

    Zinc reacts with dilute hydrochloric acid: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

    1. (a)

      Name the product that is a gas.

      [1]
    2. (b)

      State why the symbol equation is described as balanced.

      [1]
    3. (c)

      Calculate the relative formula mass of hydrochloric acid, HCl. (Aᵣ: H = 1, Cl = 35.5)

      [2]
  2. 12

    A student makes copper(II) sulfate by reacting 0.050 mol of copper(II) oxide with an excess of dilute sulfuric acid: CuO + H₂SO₄ → CuSO₄ + H₂O

    1. (a)

      Calculate the mass of 0.050 mol of copper(II) oxide. (Mᵣ of CuO = 80)

      [2]
    2. (b)

      Deduce the amount, in moles, of copper(II) sulfate produced.

      [1]
    3. (c)

      Calculate the mass of copper(II) sulfate produced. (Mᵣ of CuSO₄ = 160)

      [2]
    4. (d)

      State why the dilute sulfuric acid is used in excess.

      [1]
  3. 13

    20.0 cm³ of 0.100 mol/dm³ sodium hydroxide solution is neutralised by 0.100 mol/dm³ hydrochloric acid: NaOH + HCl → NaCl + H₂O

    1. (a)

      Calculate the amount, in moles, of sodium hydroxide in 20.0 cm³ of 0.100 mol/dm³ solution.

      [2]
    2. (b)

      Deduce the volume of 0.100 mol/dm³ hydrochloric acid needed to reach the end-point.

      [2]
    3. (c)

      State the pH of the neutral solution formed at the end-point.

      [1]
  4. 14

    Ammonia is made from nitrogen and hydrogen: N₂ + 3H₂ ⇌ 2NH₃

    1. (a)

      2.0 mol of ammonia is produced. Calculate its volume at room temperature and pressure. (molar gas volume = 24 dm³)

      [2]
    2. (b)

      The theoretical yield is 68 g of ammonia (Mᵣ = 17) but only 51 g is actually obtained. Calculate the percentage yield.

      [2]
    3. (c)

      State one reason why the actual yield may be less than the theoretical yield.

      [1]

— End of paper —