Chem208_Lecture_26_BW - cell (assume volume is 1.0 liter in...

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1 Among the participants: Prof. John Terry (3-3:30PM) Prof. Thomas Ruttledge (2:30-3PM) Feeling Stressed?
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2 Today: Electrochemistry (Ch. 20) - Galvanic Cells - Read section 20-5 (Batteries) PS10 is due Friday, 4/25, at 2:00 PS11 can be downloaded or picked up today
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4 Cell Potential under any conditions: The Nernst Equation G = -nFE and G = G° + RTlnQ E = E° – RT / nF lnQ
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5 Start with the standard Cu/Ag cell. Allow a current of 5.0 amp to flow for 2.0 hours. (1 amp = 1 coulomb/sec) Calculate: (a) the change in mass for each electrode and (b) the cell potential, E
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Unformatted text preview: cell (assume volume is 1.0 liter in each compartment) after the two hours have passed. 6 Concentration Cells Consider the cell: Ag (s) | Ag + (0.01M) || Ag + (1.0M) | Ag (s) Anode half reaction: Ag (s) Ag + (0.01 M) + e Overall cell reaction: Ag + (1.0 M) Ag + (0.01 M) Cathode half reaction: Ag (1.0 M) + e Ag (s) E = 0.00 volt 7 Calculate K sp for AgI (s) given the following: E cell = 0.416 volt for: Ag (s) | Ag + (satd AgI) || Ag + (0.1 M) | Ag(s) Overall cell reaction: Ag (0.1 M) Ag + (? M)...
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This note was uploaded on 03/29/2009 for the course CHEM 2080 taught by Professor Davis,f during the Spring '07 term at Cornell University (Engineering School).

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Chem208_Lecture_26_BW - cell (assume volume is 1.0 liter in...

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