Unit 5: Reactivity 2: How Much, How Fast and How Far?
Topic 5.1: How Much? The Amount of Chemical Change Questions
Practice 20 exam-style questions for IB Chemistry Topic 5.1. Review the question stems below, then unlock the full Question Bank to access markschemes, model answers, and AI grading.
1State1 mark
2026
State what is meant by the end point of a titration.
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2026
Draw a labelled diagram of the apparatus used for a titration.
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2026
State what the state symbols (s), (l), (g) and (aq) represent.
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Unlock Question4Deduce3 marks
Hydrogen reacts with chlorine: H₂ + Cl₂ → 2HCl.
A mixture of 0.30 mol of hydrogen and 0.20 mol of chlorine is allowed to react.
Deduce the limiting reactant and state the amount, in moles, of hydrogen chloride formed. [3]
A mixture of 0.30 mol of hydrogen and 0.20 mol of chlorine is allowed to react.
Deduce the limiting reactant and state the amount, in moles, of hydrogen chloride formed. [3]
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Unlock Question5Calculate2 marks
50 cm³ of butane, C₄H₁₀, is burned completely. All gas volumes are measured at the same temperature and pressure (with water as a liquid). Calculate the volume of carbon dioxide produced. [2]
2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(l)
2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(l)
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Unlock Question6calculate3 marks
In a titration, 24.20 cm³ of 0.100 mol dm⁻³ sodium hydroxide neutralises 25.00 cm³ of hydrochloric acid. Calculate the concentration of the acid. NaOH + HCl → NaCl + H₂O
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21.50 cm³ of 0.200 mol dm⁻³ sodium hydroxide is needed to neutralise 25.00 cm³ of sulfuric acid. Calculate the concentration of the sulfuric acid. H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O
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Unlock Question8explain2 marks
Explain why a titration is repeated until concordant titres are obtained, and state what makes titres concordant.
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Balance the equation for the complete combustion of propane: C₃H₈ + O₂ → CO₂ + H₂O, and state the total number of moles of gas on each side.
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Write a balanced equation, including state symbols, for the reaction of solid calcium carbonate with aqueous hydrochloric acid.
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Explain why a chemical equation must be balanced, and state what is conserved in a chemical reaction.
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Magnesium reacts with hydrochloric acid: Mg + 2HCl → MgCl₂ + H₂. Calculate the amount, in mol, of hydrochloric acid needed to react completely with 0.100 mol of magnesium, and the amount of hydrogen produced.
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Unlock Question13define3 marks
Define limiting reactant and state how it can be identified when the masses of both reactants are known.
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6.00 g of magnesium is burned in 4.00 g of oxygen: 2Mg + O₂ → 2MgO. Determine the limiting reactant. (M: Mg 24.31, O₂ 32.00)
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Unlock Question15calculate2 marks
Using the same reaction, 2Mg + O₂ → 2MgO with magnesium limiting at 0.2468 mol, calculate the maximum mass of magnesium oxide formed. (M(MgO) = 40.31 g mol⁻¹)
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A reaction has a theoretical yield of 15.0 g but 12.6 g of product is obtained. Calculate the percentage yield.
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For the fermentation C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂, calculate the atom economy for ethanol. (M: C₆H₁₂O₆ 180.18, C₂H₅OH 46.07, CO₂ 44.01)
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Explain the difference between percentage yield and atom economy, and state which is fixed by the balanced equation alone.
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Give two reasons why the percentage yield of a reaction carried out in a school laboratory is usually less than 100%.
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Calculate the volume of carbon dioxide, in dm³, produced at STP when 2.00 mol of calcium carbonate decomposes: CaCO₃ → CaO + CO₂. (Molar volume at STP = 22.7 dm³ mol⁻¹)
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