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TAMU CHEM 362 - Lecture 13 - Redox Reactions

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Electrochemistry Redox ReactionsSlide Number 2Slide Number 3Hydrogen Fuel CellsSlide Number 5Slide Number 6A zinc/acid batteryDaniell Cell. Copper Deposition/Zinc DissolutionSlide Number 9Slide Number 10Slide Number 11Slide Number 12Slide Number 13Lead Acid BatteryLithium BatteriesSlide Number 16Lithium Ion BatteryLithium Ion Battery: The ElectrochemistrySlide Number 19Electrochemistry Redox ReactionsInorganic Chemistry Chapter 1: Figure 5.17 Redox © 2009 W.H. Freeman Redox ReactionsInorganic Chemistry Chapter 1: Box 5.1 © 2009 W.H. FreemanHydrogen Fuel Cells 2H24H+ + 4e-AnodeCathode4H+ + 4e- + O22H2OOverall2H2 + O22H2OAlternate Sources of Energy Specific Energy (MJ/Kg) Uranium-235 83,140,000 Hydrogen 123 Gasoline 46 Propane 46 Fat 37 Coal 24 Carbohydrates 17 Platinum is currently the best catalyst for both the production and oxidation of hydrogen. TOF = 6,000 s-1 Platinum: $51,076.75 per kg Iron: $0.20 per kg Nickel: $2.94 per kg 2H24H+ + 4e-AnodeCathode4H+ + 4e- + O22H2OOverall2H2 + O22H2Ohttp://www.keepbanderabeautiful.org 5Inorganic Chemistry Chapter 1: Figure 5.1 Galvanic © 2009 W.H. Freeman Galvanic Cells: Harness the energy within chemical redox processes, converting it into Electrical EnergyA zinc/acid batteryDaniell Cell. Copper Deposition/Zinc DissolutionInorganic Chemistry Chapter 1: Figure 5.2 © 2009 W.H. FreemanInorganic Chemistry Chapter 1: Table 5.1 © 2009 W.H. FreemanInorganic Chemistry Chapter 1: Table 5.2 © 2009 W.H. FreemanLead Acid Battery Overall Reaction: a “comproportionation reaction”Lithium Batteries • Disposable • Produce voltages from 1.5 V to about 3.7 V. • (comparable to a zinc–carbon or alkaline battery)Lithium Ion BatteriesLithium Ion BatteryLithium Ion Battery: The ElectrochemistryLithium Ion Batteries:


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TAMU CHEM 362 - Lecture 13 - Redox Reactions

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