lec 4 chem 6c

lec 4 chem 6c - Review Nernst Equation = 0.02568V lnQ n...

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Review: Nernst Equation: Applications of Galvanic cells ξ = ξ ° - 0.02568V lnQ n Note: If you are having trouble with the overall cell potential, visit my website
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Cathodic Protection Electrolysis Preview: Chemical Kinetics Rates of decomposition and formation Total reaction rates
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Why doesn’t the USS Ronald Regan Rust?
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Cathodic Protection An underground Pipe Moist, electrolytic soil Cathode Mg Conductive wire Anode The Mg is a better reducing agent than Fe, it gets attacked (oxidized) before Fe Navy ships use Ti
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Electrolysis The use of electrical energy to produce a chemical change (cell potential is negative) Applying a voltage (bias) to a galvanic cell that is higher than the cell potential will create an electrolytic cell. (reverse of a galvanic cell)
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Electrolysis of water Anode: 2H 2 O O 2 + 4H + + 4e - Cathode: 4H 2 O + 4e - 2H 2 + 4OH - Net reaction: 6H 2 O 2H 2 + O 2 + 4(H + + OH - ) 4H 2 O Or 2H 2 O 2H 2 + O 2
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Using a 6V battery you can make H 2 and O 2 ! Water is oxidized Water is reduced
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Chapter 13 : Chemical Kinetics Chemical Kinetic The study of reaction rates Thus far we have only dealt with thermodynamics: the spontaneity of a reaction Kinetics tells us how fast (or slow) the reaction will proceed
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thermodynamically unstable by 2 kJ, but doesn’t turn into graphite because it is kinetically hindered. No observable change in
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This note was uploaded on 03/21/2009 for the course CHEM 6C taught by Professor Hoeger during the Spring '08 term at UCSD.

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lec 4 chem 6c - Review Nernst Equation = 0.02568V lnQ n...

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