Chapter 8: Energy from Electron Transfer

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1 Chapter 8: Energy from Electron Transfer In his 2006 State of the Union address, President George W. Bush proclaimed... we are addicted to oil Are we doomed as a country to go on to the bitter end in terms of our addiction to oil?

2 A battery is a system for the direct conversion of chemical energy to electrical energy. Batteries are found everywhere in today s society because they are convenient, transportable sources of stored energy. The batteries shown here are more correctly called galvanic cells. A series of galvanic cells that are wired together constitutes a true battery like the one in your car. 8.1

3 A galvanic cell is a device that converts the energy released in a spontaneous chemical reaction into electrical energy. Chemical to electrical energy This is accomplished by the transfer of electrons from one substance to another. Consider a nickel-cadmium (NiCad) battery: Electrons are transferred from cadmium to nickel. 8.1

4 The electron transfer process involves two changes: the cadmium is oxidized, and the nickel is reduced. Each process is expressed as a half-reaction: Oxidation half-reaction: Cd Cd e Reduction half-reaction: 2 Ni e 2 Ni 2+ Overall cell reaction: 2 Ni 3+ + Cd 2 Ni 2+ + Cd 2+ The cadmium releases two electrons, resulting in a 2+ ion. Two Ni 3+ ions accept the two electrons and their respective charges go from 3+ to 2+. The overall cell reaction does not have any electrons written in it-they must cancel. 8.1

5 Oxidation is loss of electrons: Cd Cd e Cd loses electrons Reduction is gain of electrons : 2 Ni e 2 Ni 2+ Ni 3+ gains electrons Oil Rig is a useful mnemonic device The transfer of electrons through an external circuit produces electricity, the flow of electrons from one region to another that is driven by a difference in potential energy. 8.1

6 To enable this transfer, electrodes (electrical conductors) are placed in the cell as sites for chemical reactions. Reduction occurs at the cathode The cathode receives the electrons. Oxidation occurs at the anode The difference in electrochemical potential between the two electrodes is the voltage (units are in volts). 8.1

7 A Laboratory Galvanic Cell Oxidation (at anode): Zn (S) Zn 2+ (aq) Reduction (at cathode): Cu 2+ (S) Zn 2+ (aq) 8.1

8 An Alkaline Cell 8.2

9 Mercury batteries had the advantage of being very small Used in watches, cameras, hearing aids Toxicity and disposal concerns led to alternatives 8.2

10 Lead-Acid Storage Batteries This is a true battery as it consists of a series of six cells. Anode = Pb Cathode = PbO 2 Rechargable: Pb(s) + PbO 2 (s) + 2 H 2 SO 4 (aq) discharging re-charging 2 PbSO 4 (s) + 2 H 2 O(l) 8.3

11 Hybrid Vehicles Combining the use of gasoline and battery technology Many hybrids, unlike conventional gasoline-powered cars, deliver better mileage in city driving than at highway speeds. 8.4

12 A fuel cell is a galvanic cell that produces electricity by converting the chemical energy of a fuel directly into electricity without burning the fuel. Both fuel and oxidizer must constantly flow into the cell to continue the chemical reaction. 8.5

13 Chemical Changes in a Fuel Cell H 2 + ½ O 2 H 2 O Anode reaction: (Oxidation half-reaction) H 2 (g) 2 H + (aq) + 2 e Cathode reaction: (Reduction half-reaction) ½ O 2 (g) + 2 H + (aq) + 2 e - H 2 O(l) Overall (sum of the half-reactions) H 2 (g) + ½ O 2 (g) + 2 H + (aq) + 2 e - 2 H + (aq) + 2 e - + H 2 O(l) Net equation: H 2 (g) + ½ O 2 (g) H 2 O(l) 8.5

14 Comparing Combustion with Fuel Cell Technology Process Reactants Products Comments Traditional Combustion Fuel: gasoline, hydrocarbons, ethanol, wood, ect. Oxidant: O 2 (from air) H 2 O, heat, light, sound; CO 2 and CO (greenhouse gases) Rapid process, flame present, lower efficiency, best process for producing heat Fuel Cell Technology Fuel: H 2 Oxidant: O 2 (from air) H 2 O, electricity, some heat Slower process, no flame, quiet and more efficient, best for generating electricity 8.5

15 Fuel Cell Autos Slim solid oxide fuel cell 8.6

16 If the Hydrogen Economy becomes reality, where will we get the H 2? Hydrogen (and oxygen) gas produced by the electrolysis of water. But this process requires energy. 8.7

17 The Hydrogen Economy: New Potential Sources of Hydrogen A computer simulation of hydrogen molecules (red) absorbed onto both the interior and exterior of a collection of carbon nanotubes (blue). Certain algae produce H 2 Via photosynthesis-very promising technology. Realistic future? 8.8

18 Photovoltaic Cells Energy of the future? An awesome source of energy. Our society has been using photovoltaic cells (solar cells) at a minimum level, but will we all begin picking up on this natural form of energy as a way to conserve our natural coal and petroleum supply? Thin wafers of ultra pure Si used for voltaic cells. 8.9

19 Other countries making use of solar energy Solar Park Gut Erlasee in Bavaria. At peak capacity, it can generate 12 MW. It s time to make important decisions and advances in alternative energy technology and new sources of renewable energy. Harnessing the energy of the sun for pumping water 8.10

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