CHEM 1415 1st EditionLecture 20Unit: Corrosion, Batteries Outline of Current Lecture I. CorrosionII. BatteriesIII. Primary CellsIV. Secondary CellsV. Fuel CellsCurrent Lecture Corrosiono Degradation of metals by chemical reactions with the environment, slow combination of oxygen with metals to form oxideso Uniform corrosion – most visible forms, ie rusting of automobileso Galvanic corrosion – occurs when two different metals contact each other in the presence of an appropriate electrolyteo Crevice corrosion – degradation of the gap between two metals Batterieso A cell or series of cells that generates an electric currento Provide a means to harness the electrical work of a galvanic cell Primary Cellso Single use batteries that cannot be rechargedo Most common is alkaline batterieso Mercury batteries are small primary cell batteries with a long lasting lifetime Secondary Cellso Rechargeable batterieso Nickel-cadmium batteries – popular in cellphones, digital cameras, and smaller computer deviceso Lead-acid battery Generates a potential of 2.0 V Rechargeable because lead sulfate product tends to adhere to the electrode surfaces Eventually the lead sulfate falls away from the electrodes and it cannot be recharged Fuel CellsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.o Voltaic cell in which the reactants can be supplied continuously and the products of the cell reaction are continuously removedo Uses chemical reaction to produce electrical energyo Can be refueled on an ongoing basiso Most common is the reaction of hydrogen and oxygen to produce
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