Redox Equilibria · CAPE Chemistry Unit 1

45 past-paper questions on Redox Equilibria, part of Kinetics and Equilibria, from every CAPE Chemistry Unit 1 paper on Quelpr.

1. 2(d)(i)2 marks· CAPE Chemistry Unit 1 · May/June 2022 · Paper 2Define the term 'standard electrode potential of a half cell'.
2. 2(d)(ii)5 marks· CAPE Chemistry Unit 1 · May/June 2022 · Paper 2Draw a labelled diagram to show how the standard electrode potential of the Fe3+(aq)/Fe2+(aq) half cell can be determined.
3. 2(c)(i)3 marks· CAPE Chemistry Unit 1 · May/June 2023 · Paper 2Figure 1 is a diagram of a voltaic cell. Give the correct labels that correspond to the letters A, B and C on the voltaic cell.
4. 2(c)(ii)1 mark· CAPE Chemistry Unit 1 · May/June 2023 · Paper 2Describe an observation expected during electrolysis.
5. 2(c)(iii)1 mark· CAPE Chemistry Unit 1 · May/June 2023 · Paper 2Describe an observed change if the cell components are based on the cell type Zn(s) | Zn²⁺(aq) || Cu²⁺(aq) | Cu(s).
6. 2(c)(iv)1 mark· CAPE Chemistry Unit 1 · May/June 2023 · Paper 2State a chemical compound which is in the salt bridge.
7. 3(g)(i)1 mark· CAPE Chemistry Unit 1 · May/June 2023 · Paper 2Which of the halogens bring about the maximum change in oxidation number of sulfur?
8. 3(g)(ii)1 mark· CAPE Chemistry Unit 1 · May/June 2023 · Paper 2Write ONE full ionic equation to represent this change.
9. 2(e)(i)2 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Define standard cell potential.
10. 2(e)(ii)2 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Define standard electrode potential.
11. 2(f)5 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Describe, in detail, the steps that could be used to determine the standard electrode potential of copper in the laboratory.
12. 2(a)2 marks· Chemistry · Unit 1 Q2 2(a)Define the term 'standard electrode potential'.
13. 2(a)(i)5 marks· Chemistry · Unit 1 Q2 2(a)(i)Outline the experimental steps he has to follow to obtain a reading of approximately 1.10 V on his voltmeter.
14. 2(a)(i)2 marks· Chemistry · Unit 1 Q2 2(a)(i)Define the term: Standard electrode potential of a half-cell
15. 2(a)(i)2 marks· Chemistry · Unit 1 Q2 2(a)(i)Define EACH of the following terms: Standard electrode potential of a half-cell
16. 2(a)(ii)2 marks· Chemistry · Unit 1 Q2 2(a)(ii)Define the term: Standard cell potential of an electrochemical cell
17. 2(a)(ii)2 marks· Chemistry · Unit 1 Q2 2(a)(ii)Write the ionic half equation for the reaction occurring at EACH of the electrodes.
18. 2(a)(ii)2 marks· Chemistry · Unit 1 Q2 2(a)(ii)Define EACH of the following terms: Standard cell potential of an electrochemical cell
19. 2(a)(iii)1 mark· Chemistry · Unit 1 Q2 2(a)(iii)Identify the anode and the cathode.
20. 2(a)(iv)1 mark· Chemistry · Unit 1 Q2 2(a)(iv)Explain the direction of electron flow.
21. 2(a)(v)1 mark· Chemistry · Unit 1 Q2 2(a)(v)Write the cell diagram.
22. 2(a)(vi)1 mark· Chemistry · Unit 1 Q2 2(a)(vi)Write the equation to represent the cell reaction.
23. 2(b)2 marks· Chemistry · Unit 1 Q2 2(b)Identify the parts of the standard hydrogen electrode labelled A and B in Figure 2.
24. 2(b)2 marks· Chemistry · Unit 1 Q2 2(b)Use the Eº value for each electrode (in the data booklet) to determine the Eºcell.
25. 2(b)(i)2 marks· Chemistry · Unit 1 Q2 2(b)(i)Write the ionic half-equation for the reaction taking place at EACH of the electrodes. ANODE: CATHODE:
26. 2(b)(i)a)5 marks· Chemistry · Unit 1 Q2 2(b)(i)a)On the diagram in Figure 1, label the ions in Solution A and Solution B
27. 2(b)(i)b)1 mark· Chemistry · Unit 1 Q2 2(b)(i)b)On the diagram in Figure 1, label the salt bridge
28. 2(b)(i)c)1 mark· Chemistry · Unit 1 Q2 2(b)(i)c)On the diagram in Figure 1, label the cathode and anode
29. 2(b)(i)d)1 mark· Chemistry · Unit 1 Q2 2(b)(i)d)On the diagram in Figure 1, label the direction of electron flow.
30. 2(b)(ii)1 mark· Chemistry · Unit 1 Q2 2(b)(ii)Write the cell diagram.
31. 2(b)(ii)1 mark· Chemistry · Unit 1 Q2 2(b)(ii)State what would be observed at the cathode after the electrochemical cell in Figure 1 has been running for a few hours.
32. 2(b)(iii)6 marks· Chemistry · Unit 1 Q2 2(b)(iii)Draw a well-labelled diagram of the electrochemical cell. Indicate the direction of electron flow.
33. 2(b)(iii)2 marks· Chemistry · Unit 1 Q2 2(b)(iii)State the experimental conditions used in the preparation of the cell in Figure 1. Temperature, Concentration of Solutions A and B
34. 2(b)(iv)2 marks· Chemistry · Unit 1 Q2 2(b)(iv)For EACH electrode shown in Table 2, select the Eº value to determine the Ecell.
35. 2(b)(iv)3 marks· Chemistry · Unit 1 Q2 2(b)(iv)Use the information in your Data Booklet to calculate the standard cell potential, Ecell, for the electrochemical cell in Figure 1.
36. 2(c)2 marks· Chemistry · Unit 1 Q2 2(c)Suggest TWO changes which could be made to the cell in (a) to cause the cell potential to be greater than 1.10V.
37. 2(c)(i)4 marks· Chemistry · Unit 1 Q2 2(c)(i)Construct a labelled diagram to represent this cell and indicate the direction of electron flow when the cell is operating.
38. 2(c)(ii)2 marks· Chemistry · Unit 1 Q2 2(c)(ii)Write the relevant equations to represent the change taking place at the anode and the cathode. Anode: Cathode:
39. 2(c)(iii)2 marks· Chemistry · Unit 1 Q2 2(c)(iii)Write the balanced equation for the OVERALL cell reaction.
40. 2(c)(iv)1 mark· Chemistry · Unit 1 Q2 2(c)(iv)Refer to the data booklet to calculate the standard cell potential.
41. 2(d)2 marks· Chemistry · Unit 1 Q2 2(d)List TWO types of energy storage devices.
42. 181 mark· Chemistry · Unit 1 Q18 18In a standard hydrogen half-cell, a platinum electrode is used to
43. 181 mark· Chemistry · Unit 1 Q18 18In a standard hydrogen half-cell, a platinum electrode is used to
44. 301 mark· Chemistry · Unit 1 Q30 30The standard electrode potential of tin (Sn) is Sn²⁺(aq) + 2e⁻ → Sn(s), E° = -0.14 V. In which of the following equations is the metal UNABLE to reduce Sn²⁺?
45. 301 mark· Chemistry · Unit 1 Q30 30In which of the following equations is the metal UNABLE to reduce Sn²⁺?