Electrochemistry Chapter 17 Exam Questions

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Chapter 17: Electrochemistry

1. Write a balanced redox reaction for the formation of rust on iron metal and identify the correct oxidizing agent and/or reducing agent. (Outcome # 6) (DOK 3)
2. Iron is the oxidizing agent and O₂ is neither a reducing agent nor an oxidizing agent
3. Iron is the oxidizing agent and O₂ is the reducing agent
4. Iron is the reducing agent and O₂ is the oxidizing agent
5. Which is the reducing agent in the combustion of methanol? (Outcome # 6) (DOK 3)
6. CH₃OH
7. O₂
8. CO₂
9. Which is the oxidizing agent in the combustion of methanol? (Outcome # 6) (DOK 3)
10. CH₃OH
11. O₂
12. CO₂
13. Propane is used as a fuel source on many barbeque grills. What is undergoing oxidation during the burning of propane while grilling? (Outcome # 6) (DOK 3)
14. CH₃CH₂CH₃
15. O₂
16. CO₂
17. Propane is used as a fuel source on many barbeque grills. What is undergoing reduction during the burning of propane while grilling? (Outcome # 6) (DOK 3) (Paired item 1)
18. CH₃CH₂CH₃
19. O₂
20. CO₂
21. Automobiles from northern states tend to show more signs of rust formation than southern states. The reason for this is that the rate of corrosion is affected by _____, which is more common during winter months especially in northern states. (Outcome # 6) (DOK 1)
22. the cold air and clouds
23. rain clouds
24. snow, ice, and salt mixtures
25. Certain anaerobic organisms such as methanogens have the ability to metabolize carbon dioxide into methane in the presence of hydrogen. Methane is produced by the oxidation of _____? (Outcome # 6) (DOK 3)
26. H₂
27. CO₂
28. CH₄
29. A voltaic cell must be split into two separate cells, an oxidation and reduction half-cells. The two half-cells must be connected by a _____ so ions can freely flow between the two half-cells to balance the charges or the voltaic cell cannot function. (Outcome # 10) (DOK 2)
30. metallic wire
31. salt bridge
32. membrane
33. In a voltaic cell, oxidation occurs at the _____. (Outcome # 10) (DOK 1)
34. anode terminal
35. cathode terminal
36. positive terminal
37. In a voltaic cell, reduction occurs at the _____. (Outcome # 10) (DOK 1)
38. anode terminal
39. cathode terminal
40. negative terminal
41. Electron flow in a voltaic cell is always from _____ to _____. (Outcome # 10) (DOK 2)
42. anode to cathode
43. cathode to anode
44. anode to negative terminal
45. The following can be used as an electrolyte for a salt bridge in a voltaic cell? (Outcome # 10) (DOK 1)
46. KNO₃(aq)
47. H₂O(l)
48. CH₃OH(l)
49. The following can be used as an electrolyte for a salt bridge in a voltaic cell? (Outcome # 10) (DOK 1) (Paired item 1)
50. CCl₄(l)
51. CH₃CH₂OH(l)
52. Na₂SO₄(aq)
53. In a voltaic cell, electrons are produced at the _____. (Outcome # 10) (DOK 1)
54. positive terminal
55. anode terminal
56. cathode terminal
57. The anode terminal in a voltaic cell is the _____ terminal. (Outcome # 10) (DOK 1)
58. (-)
59. (+)
60. Neutral
61. The cathode terminal in a voltaic cell is the _____ terminal. (Outcome # 10) (DOK 1)
62. (-)
63. (+)
64. neutral
65. In a voltaic cell, electrons are received at the _____. (Outcome # 10) (DOK 1)
66. cathode terminal
67. negative terminal
68. anode terminal
69. Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Zn(s) + Cu²⁺(aq) 🡪 Zn²⁺(aq) + Cu(s)? (Outcome # 11) (DOK 2)

E°_red = -0.763 V for Zn²⁺(aq) + 2e^- 🡪 Zn(s)

E°_red = +0.340 V for Cu²⁺(aq) + 2e^- 🡪 Cu(s)

1. +1.103 V
2. -0.423 V
3. +0.423 V
4. Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Cu(s) + 2Ag⁺ 🡪 Cu²⁺(aq) + 2Ag(s)? (Outcome # 11) (DOK 2) (Paired item 1)

E°_red = +0.800 V for Ag⁺(aq) + e^- 🡪 Ag(s)

E°_red = +0.340 V for Cu²⁺(aq) + 2e^- 🡪 Cu(s)

1. +1.14 V
2. +0.460 V
3. +1.26 V
4. Based on the following reduction potential data, which is the strongest reducing agent? (Outcome # 11) (DOK 1)

E°_red = +1.78 V for H₂O₂(aq) + 2H⁺(aq) + 2e- 🡪 2H₂O(l)

E°_red = +0.800 V for Ag⁺(aq) + e^- 🡪 Ag(s)

E°_red = -0.130 V for Pb²⁺(aq) + 2e^- 🡪 Pb(s)

1. Pb(s)
2. Ag(s)
3. H₂O(l)
4. Based on the following reduction potential data, which is the strongest oxidizing agent? (Outcome # 11) (DOK 1)

E°_red = +1.78 V for H₂O₂(aq) + 2H⁺(aq) + 2e^- 🡪 2H₂O(l)

E°_red = +0.800 V for Ag⁺(aq) + e^- 🡪 Ag(s)

E°_red = -0.130 V for Pb²⁺(aq) + 2e^- 🡪 Pb(s)

1. Pb²⁺(aq)
2. H₂O₂(aq)
3. Ag⁺(aq)
4. The standard cell potential is +0.460 V for the following electrochemical cell reaction: Cu(s) + 2Ag⁺(aq) 🡪 Cu²⁺(aq) + 2Ag(s). What is the ∆G°_rxn? (Outcome # 11) (DOK 2)
5. -88.8 kJ/mol
6. -44.4 kJ/mol
7. +44.4 kJ/mol
8. What is the ∆G°_rxn for a 2 electron transfer electrochemical cell with a standard cell potential of +0.770 V. (Outcome # 11) (DOK 2)
9. -74.3 kJ/mol
10. -149 kJ/mol
11. +74.3 kJ/mol
12. Based on the following reduction potential data, what is the ∆G°_rxn for the following electrochemical cell reaction: Zn(s) + Cu²⁺(aq) 🡪 Zn²⁺(aq) + Cu(s)? (Outcome # 11) (DOK 3)

E°_red = -0.763 V for Zn²⁺(aq) + 2e^- 🡪 Zn(s)

E°_red = +0.340 V for Cu²⁺(aq) + 2e^- 🡪 Cu(s)

1. +106 kJ/mol
2. -106 kJ/mol
3. -213 kJ/mol
4. Which of the following acids is a strong oxidant? (Outcome # 5) (DOK 1)
5. HCl
6. HNO₃
7. HI
8. Which strong acid is commonly used in automobile batteries? (Outcome # 2) (DOK 2)
9. HCl
10. H₂SO₄
11. HNO₃
12. Cell phones batteries are typically rechargeable. How do they differ from non-rechargeable batteries? (Outcome # 2) (DOK 3)
13. A rechargeable battery has the ability to undergo a double replacement reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.
14. A rechargeable battery has the ability to undergo a reversible redox reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.
15. A rechargeable battery has the ability to undergo a redox reaction while non-rechargeable batteries do not. Therefore, the reverse direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.
16. The process of corrosion involves what type of reaction? (Outcome # 2) (DOK 2)
17. double displacement reaction
18. acid-base reaction
19. redox reaction
20. What is the oxidation state of oxygen in K₂O₂? (Outcome # 2) (DOK 2)
21. 0
22. -1
23. -2
24. Which of the following is a strong oxidizing agent? (Outcome # 2) (DOK 2)
25. N₂
26. O₂
27. H₂