Scottish Highers · Higher Chemistry

Rates, Bonding and Quantities

37 practice questions, each with the answer and an explanation.

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Random questions from this topic, one at a time. You see the answer and the explanation straight after each one.

All 37 questions

  1. What is the name given to a substance that speeds up a reaction without being used up?
  2. Why does increasing the temperature increase the rate of a reaction?
  3. What is the electron arrangement of a sodium atom (atomic number 11)?
  4. Which type of bonding is found in sodium chloride?
  5. Which statement explains why metals conduct electricity?
  6. Why does water have a higher boiling point than hydrogen sulfide?
  7. What is the mass of one mole of calcium carbonate (CaCO3)? (Ca = 40, C = 12, O = 16)
  8. How many moles are in 5.6 g of iron? (Fe = 56)
  9. In the reaction 2H2 + O2 gives 2H2O, how many grams of water are formed from 4 g of hydrogen? (H = 1, O = 16)
  10. What is the pH of a solution with a hydrogen ion concentration of 0.001 mol per litre?
  11. Which is a property of an acid?
  12. What type of reaction takes place when an acid reacts with an alkali?
  13. What volume of 0.5 mol per litre sodium hydroxide neutralises 25 cm3 of 0.2 mol per litre hydrochloric acid?
  14. Which statement is true for an exothermic reaction?
  15. Which statement explains why the first ionisation energy increases across a period?
  16. Why does the first ionisation energy decrease down a group?
  17. Which type of bond is present in a molecule of hydrogen chloride, given electronegativities of H = 2.2 and Cl = 3.2?
  18. Why does hydrogen fluoride (HF) have a higher boiling point than hydrogen chloride (HCl)?
  19. Why do the boiling points of the noble gases increase down Group 0?
  20. Which species acts as an oxidising agent in the reaction Zn + Cu²⁺ → Zn²⁺ + Cu?
  21. In which half-equation is the species oxidised?
  22. 25.0 cm³ of an acidified solution of iron(II) ions is titrated with 0.0200 mol/l potassium manganate(VII). 20.0 cm³ is needed. The equation is MnO₄⁻ + 8H⁺ + 5Fe²⁺ → Mn²⁺ + 4H₂O + 5Fe³⁺. What is the co…
  23. What is the percentage yield if 8.0 g of product is obtained when the theoretical yield is 12.5 g?
  24. For CaCO₃ → CaO + CO₂ (GFM CaCO₃ = 100, CaO = 56), what is the atom economy for making CaO?
  25. A hydrocarbon contains 85.7% carbon and 14.3% hydrogen by mass. What is its empirical formula? (C = 12, H = 1)
  26. Given the enthalpy changes C(s) + O₂(g) → CO₂(g) ΔH = −394 kJ/mol and CO(g) + ½O₂(g) → CO₂(g) ΔH = −283 kJ/mol, what is ΔH for C(s) + ½O₂(g) → CO(g)?
  27. Use bond enthalpies (C–H 413, O=O 498, C=O 805, O–H 464 kJ/mol) to find ΔH for CH₄ + 2O₂ → CO₂ + 2H₂O.
  28. 0.50 g of ethanol heats 100 g of water from 20.0 °C to 31.0 °C. (c = 4.18 kJ/kg/°C). What is the energy released?
  29. Which change would increase the equilibrium yield of ammonia in N₂(g) + 3H₂(g) ⇌ 2NH₃(g)?
  30. What does a catalyst do to the position of equilibrium?
  31. On a Maxwell–Boltzmann distribution, what is the effect of raising the temperature?
  32. The time taken for a reaction to finish halves when the temperature is raised. What happens to the relative rate?
  33. 0.50 g of ethanol (GFM 46) is burned and the heat raises the temperature of 100 g of water by 11.0 °C (c = 4.18 kJ/kg/°C). What is the enthalpy of combustion of ethanol, per mole?
  34. 25.0 cm³ of sulfuric acid is neutralised by 30.0 cm³ of 0.100 mol/l sodium hydroxide: H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O. What is the concentration of the acid?
  35. 4.6 g of ethanol (GFM 46) reacts with excess ethanoic acid to make ethyl ethanoate (GFM 88). 6.6 g of ester is obtained. What is the percentage yield?
  36. In acid, dichromate ions are reduced: Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O. How many moles of iron(II) ions (Fe²⁺ → Fe³⁺ + e⁻) are oxidised by 0.0100 mol of dichromate?
  37. The atom economy for making ethene by the reaction C₂H₅OH → C₂H₄ + H₂O is closest to which value? (GFM C₂H₅OH = 46, C₂H₄ = 28)

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