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1. Ni-cad batteries are rechargeable. The two reduction half-cells involved in the Ni-cad batteries Cd(OH)2 (s) + 2 e Cd (s) + 2OH(aq) Eº = -0.860 V are: (a) (b) NiO2 (s) + 2 H₂O (1) + 2e → Ni(OH)2 (s) + 2 OH(aq) E° = 0.490 V a. Figure out which reaction must be reversed and written as an oxidation half-reaction. Write the spontaneous overall redox reaction and calculate Eºcell. b. What must serve as the anode in this battery? What serves as the cathode? c. Write the half-reactions and overall reaction that occurs when this battery is recharged. d. After charging the above battery system for 90 min. at a current of 10 mA (0.010 A), how many grams of each of the original electrodes (anode and cathode) would be produced?

1. Ni-cad batteries are rechargeable. The two reduction half-cells involved in the Ni-cad batteries Cd(OH)2 (s) + 2 e Cd (s) + 2OH(aq) Eº = -0.860 V are: (a) (b) NiO2 (s) + 2 H₂O (1) + 2e → Ni(OH)2 (s) + 2 OH(aq) E° = 0.490 V a. Figure out which reaction must be reversed and written as an oxidation half-reaction. Write the spontaneous overall redox reaction and calculate Eºcell. b. What must serve as the anode in this battery? What serves as the cathode? c. Write the half-reactions and overall reaction that occurs when this battery is recharged. d. After charging the above battery system for 90 min. at a current of 10 mA (0.010 A), how many grams of each of the original electrodes (anode and cathode) would be produced?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section17.3: Voltaic Cells
Problem 17.3PSP
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Ni-cad batteries are rechargeable. The two reduction half-cells involved in the Ni-cad batteries Cd(OH)2 (s) + 2e → Cd (s) + 2OH(aq) Eº = -0.860 V are: (a) (b) NiO2 (s) + 2 H₂O (1) + 2e → Ni(OH)2 (s) + 2OH(aq) Eº = 0.490 V a. Figure out which reaction must be reversed and written as an oxidation half-reaction. Write the spontaneous overall redox reaction and calculate Eºcell- b. What must serve as the anode in this battery? What serves as the cathode? c. Write the half-reactions and overall reaction that occurs when this battery is recharged. d. After charging the above battery system for 90 min. at a current of 10 mA (0.010 A), how many grams of each of the original electrodes (anode and cathode) would be produced? 1. 2. Pb²+ (aq) Eº = + 0.925 V? Indicate which statements are true (T) and which are false (F) for the lead-silver cell: Pb(s) 2 Ag* (s) 2 Ag (s) + + a. b. C. d. the lead electrode is the anode the standard cell notation is Ag | Ag+ (1.0M) || Pb2+ (1.0M) | Pb the reaction as written is spontaneous the lead electrode is positively charged
Transcribed Image Text:Ni-cad batteries are rechargeable. The two reduction half-cells involved in the Ni-cad batteries Cd(OH)2 (s) + 2e → Cd (s) + 2OH(aq) Eº = -0.860 V are: (a) (b) NiO2 (s) + 2 H₂O (1) + 2e → Ni(OH)2 (s) + 2OH(aq) Eº = 0.490 V a. Figure out which reaction must be reversed and written as an oxidation half-reaction. Write the spontaneous overall redox reaction and calculate Eºcell- b. What must serve as the anode in this battery? What serves as the cathode? c. Write the half-reactions and overall reaction that occurs when this battery is recharged. d. After charging the above battery system for 90 min. at a current of 10 mA (0.010 A), how many grams of each of the original electrodes (anode and cathode) would be produced? 1. 2. Pb²+ (aq) Eº = + 0.925 V? Indicate which statements are true (T) and which are false (F) for the lead-silver cell: Pb(s) 2 Ag* (s) 2 Ag (s) + + a. b. C. d. the lead electrode is the anode the standard cell notation is Ag | Ag+ (1.0M) || Pb2+ (1.0M) | Pb the reaction as written is spontaneous the lead electrode is positively charged
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