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A Level H1 Chemistry Stoichiometry Moles Quiz

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A Level H1 Chemistry From Real Exams Generated by Gemma 4 31B Updated 2026-06-03
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Questions

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A-Level Chemistry H1 Quiz - Stoichiometry Moles

Name: ________________________
Class: ________________________
Date: ________________________
Score: ________ / 45

Duration: 60 Minutes
Total Marks: 45
Instructions: Answer all questions. Show all working for calculations. Use the periodic table and formula booklet where necessary.

Section A: Foundational Calculations (Questions 1-7)

  1. Calculate the molar mass of the polymer monomer ethylene terephthalate (C₁₀H₈O₄). [1]
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  2. Determine the percentage by mass of carbon in the compound C₁₀H₈O₄. [2]
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  3. A compound contains 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. Determine its empirical formula. [2]
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  4. If the relative molecular mass of the compound in Question 3 is 180, determine its molecular formula. [1]
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  5. Calculate the number of moles of solute in 250 cm³ of a 0.150 mol dm⁻³ solution of sodium carbonate. [1]
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  6. What is the mass of 0.025 mol of anhydrous copper(II) sulfate (CuSO₄)? [2]
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  7. Calculate the volume of 0.100 mol of an ideal gas at 25.0 °C and 1.00 atm. [2]
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Section B: Application & Contextual Problems (Questions 8-14)

  1. A patient is prescribed a dosage of four 500 mg tablets of a painkiller (C₈H₉NO₂) per dose. Calculate the total mass of the active ingredient in one dose in grams. [1]
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  2. Using the information in Question 8, calculate the number of moles of the active ingredient the patient receives in one dose. [2]
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  3. A sample of magnesium carbonate (MgCO₃) is heated to decompose into MgO and CO₂. Calculate the mass of MgO produced from 5.00 g of MgCO₃. [3]
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  4. A 20.0 cm³ sample of a hydrocarbon gas is found to contain 0.0010 mol of carbon atoms. Calculate the molar volume of the gas at these conditions. [3]
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  5. A mixture of two isotopes, ¹⁰B and ¹¹B, has an average atomic mass of 10.81. Calculate the percentage abundance of ¹¹B. [3]
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  6. Calculate the mass of water of crystallization in hydrated barium chloride (BaCl₂·xH₂O) if 1.00 g of the hydrate loses 0.15 g of water upon heating. [3]
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  7. How many molecules are present in 1.50 g of glucose (C₆H₁₂O₆)? [2]
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Section C: Advanced Stoichiometry & Analysis (Questions 15-20)

  1. A 0.200 g sample of an organic acid (CₓHᵧO₂) requires 25.0 cm³ of 0.100 mol dm⁻³ NaOH for complete neutralization. Calculate the molar mass of the acid. [3]
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  2. In a reaction between 2.00 g of Al and 10.0 g of Cl₂, which reagent is in excess? [3]
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  3. Calculate the mass of AlCl₃ formed in the reaction described in Question 16. [3]
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  4. A gas cylinder contains a mixture of He and Ar. The total mass is 10.0 g and the total number of moles is 0.30 mol. Determine the mass of He in the cylinder. [4]
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  5. A 1.00 g sample of a metal carbonate (MCO₃) is reacted with excess HCl. The volume of CO₂ collected at STP is 224 cm³. Identify the metal M. [4]
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  6. A solution is prepared by dissolving 5.00 g of NaOH in water to make 250 cm³. This solution is then diluted to 500 cm³. Calculate the final concentration of the solution. [2]
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Answers

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Answer Key - Stoichiometry Moles Quiz

  1. 192 g mol⁻¹ (1012 + 81 + 4*16) [1]
  2. 62.5% ((120/192)*100) [2]
  3. CH₂O (C: 40/12=3.33, H: 6.7/1=6.7, O: 53.3/16=3.33 →\rightarrow 1:2:1) [2]
  4. C₆H₁₂O₆ (Empirical mass = 30. 180/30 = 6) [1]
  5. 0.0375 mol (0.150 * 0.250) [1]
  6. 1.60 g (0.025 * 63.5) [2]
  7. 2.45 L (or 2.45 dm³) (V = nRT/P = 0.10.0821298 / 1.00) [2]
  8. 2.00 g (4 * 500mg = 2000mg) [1]
  9. 0.0132 mol (2.00 / 151) [2]
  10. 2.83 g (n(MgCO₃) = 5/84.3 = 0.0593; n(MgO) = 0.0593; mass = 0.0593 * 40.3) [3]
  11. 20.0 dm³/mol (n = 0.001 / 1 = 0.001 mol gas; V/n = 0.020 / 0.001) [3]
  12. 80.1% (10x + 11(1-x) = 10.81 →\rightarrow 11 - x = 10.81 →\rightarrow x = 0.19; 11B = 81%) [3]
  13. x = 2 (BaCl₂·2H₂O) (n(H₂O) = 0.15/18 = 0.00833; n(salt) = 0.85/208 = 0.00408; ratio ≈\approx 2:1) [3]
  14. 2.51 x 10²¹ molecules (n = 1.5/180 = 0.00833; molecules = 0.00833 * 6.02e23) [2]
  15. 100 g mol⁻¹ (n(NaOH) = 0.025 * 0.1 = 0.0025 mol; n(acid) = 0.0025; M = 0.2 / 0.0025) [3]
  16. Chlorine (Cl₂) (n(Al) = 2/27 = 0.074; n(Cl₂) = 10/71 = 0.141. Ratio 1:1.5 needed, 1:1.9 available) [3]
  17. 4.04 g (n(AlCl₃) = n(Al) = 0.074; mass = 0.074 * 133.3) [3]
  18. 1.33 g He (4x + 40(0.3-x) = 10 →\rightarrow 4x + 12 - 40x = 10 →\rightarrow 36x = 2 →\rightarrow x = 0.0556 mol He; mass = 0.0556 * 4) [4]
  19. Calcium (Ca) (n(CO₂) = 0.224/22.4 = 0.01 mol; M(MCO₃) = 1.00/0.01 = 100; M = 100 - 60 = 40) [4]
  20. 0.200 mol dm⁻³ (n = 5/40 = 0.125; c1 = 0.125/0.25 = 0.5; c2 = 0.125/0.5 = 0.25) [2]