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Redox Reactions · CAPE Chemistry Unit 1

32 past-paper questions on Redox Reactions, part of Fundamentals in Chemistry, from every CAPE Chemistry Unit 1 paper on Quelpr.

Practise Redox Reactions
  1. 2(a)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Referring to Figure 1, explain why the chemical reaction occurring in batteries is described as a redox reaction.
  2. 2(b)(i)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Write the balanced ionic equation for the reaction that occurs, given the half-equations: SO₂(g) + 2H₂O(l) → SO₄²⁻(aq) + 2e⁻ + 4H⁺(aq) Cr₂O₇²⁻(aq) + 6e⁻ + 14H⁺ → 2Cr³⁺(aq) + 7H₂O(l)
  3. 2(b)(ii)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1State the change in oxidation number in any ONE identified reagent in the reaction.
  4. 2(c)4 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Select THREE named elements and describe an experiment, including observations, to show how the elements selected can be listed in order of oxidizing or reducing ability.
  5. 3(d)(ii)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Write the formula and state the colour of the species formed from the oxidation of Fe^2+ ions.
  6. 1(a)(i)2 marks· Chemistry · Unit 1 Q1 1(a)(i)Define the term oxidation.
  7. 1(a)(ii)2 marks· Chemistry · Unit 1 Q1 1(a)(ii)Define the term reduction.
  8. 1(b)(i)1 mark· Chemistry · Unit 1 Q1 1(b)(i)State the colour change observed.
  9. 1(b)(i)3 marks· Chemistry · Unit 1 Q1 1(b)(i)List TWO chemicals and ONE piece of apparatus that the student may use to carry out the investigation.
  10. 1(b)(ii)1 mark· Chemistry · Unit 1 Q1 1(b)(ii)Describe ONE physical change that the student may have observed.
  11. 1(b)(ii)4 marks· Chemistry · Unit 1 Q1 1(b)(ii)Given that the sulfate(IV) ion, SO₃²⁻, is converted to the sulfate(VI) ion, SO₄²⁻, in the presence of water, deduce the balanced equation for the redox reaction between Cr₂O₇²⁻(aq) and SO₃²⁻.
  12. 1(b)(ii)6 marks· Chemistry · Unit 1 Q1 1(b)(ii)Write the TWO half equations for the reaction, indicating the changes in oxidation number.
  13. 1(b)(iii)2 marks· Chemistry · Unit 1 Q1 1(b)(iii)State the roles of the two reagents, potassium manganate(VII) and hydrogen peroxide.
  14. 1(b)(iii)1 mark· Chemistry · Unit 1 Q1 1(b)(iii)Identify the oxidizing agent in (b) (ii).
  15. 1(b)(iii)1 mark· Chemistry · Unit 1 Q1 1(b)(iii)Identify the reducing agent in the experiment.
  16. 1(b)(iv)2 marks· Chemistry · Unit 1 Q1 1(b)(iv)Write relevant half equations to illustrate the chemical changes that occur with EACH element.
  17. 1(b)(v)2 marks· Chemistry · Unit 1 Q1 1(b)(v)From the half equations in (iv), deduce a balanced equation for the redox reaction.
  18. 3(b)(i)3 marks· Chemistry · Unit 1 Q3 3(b)(i)Calculate the oxidation number of vanadium in EACH of the following species: VOSO4
  19. 3(b)(ii)1 mark· Chemistry · Unit 1 Q3 3(b)(ii)Calculate the oxidation number of vanadium in EACH of the following species: VO2+
  20. 3(b)(iii)1 mark· Chemistry · Unit 1 Q3 3(b)(iii)Calculate the oxidation number of vanadium in EACH of the following species: VO2+
  21. 3(c)(i)4 marks· Chemistry · Unit 1 Q3 3(c)(i)Write half equations to explain the observation in test (b)(ii).
  22. 5(a)(i)2 marks· Chemistry · Unit 1 Q5 5(a)(i)Explain EACH of the terms 'oxidation' and 'reduction', in terms of loss and or gain of electrons
  23. 5(a)(ii)2 marks· Chemistry · Unit 1 Q5 5(a)(ii)Explain EACH of the terms 'oxidation' and 'reduction', in terms of change in oxidation number.
  24. 5(b)(i)2 marks· Chemistry · Unit 1 Q5 5(b)(i)Use the appropriate half equations (from those above) to write a balanced equation to show the reaction between hydrogen peroxide and chloric (I) (hypochlorous) acid.
  25. 5(b)(ii)6 marks· Chemistry · Unit 1 Q5 5(b)(ii)By making reference to the change in oxidation numbers of the elements in both the hydrogen peroxide AND the chloric (I) acid, determine which reactant is reduced and which is oxidised.
  26. 5(c)(i)3 marks· Chemistry · Unit 1 Q5 5(c)(i)State what type of chemical reaction occurs and write an ionic equation for the reaction.
  27. 5(c)(ii)4 marks· Chemistry · Unit 1 Q5 5(c)(ii)Which element has the greater reducing ability? Explain your answer, using a suitable half equation.
  28. 5(c)(iii)1 mark· Chemistry · Unit 1 Q5 5(c)(iii)Tin shows no reaction with solutions of EITHER iron or nickel salts. Place the elements, tin, iron and nickel in order of INCREASING reducing ability.
  29. 101 mark· Chemistry · Unit 1 Q10 10Which of the following processes represents an oxidation?
  30. 121 mark· Chemistry · Unit 1 Q12 12What is the oxidation number of chromium in EACH compound?
  31. 451 mark· Chemistry · Unit 1 Q45 45What deduction can be made from the following reactions of iodine and chlorine with sodium thiosulfate? I₂(aq) + 2S₂O₃²⁻(aq) → 2I⁻(aq) + S₄O₆²⁻(aq) 4Cl₂(aq) + S₂O₃²⁻(aq) + 5H₂O(l) → 8Cl⁻(aq) + 2SO₄²⁻(aq) + 10H⁺(aq)
  32. 451 mark· Chemistry · Unit 1 Q45 45What deduction can be made from the following reactions of iodine and chlorine with sodium thiosulfate?

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