Chem208_Lecture_26_Color - Feeling Stressed? Among the...

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Unformatted text preview: Feeling Stressed? Among the participants: □ Prof. John Terry (3-3:30PM) □ Prof. Thomas Ruttledge Ruttledge (2:30-3PM) 1 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 2 3 Cell Potential under any conditions: The Nernst Equation ∆G = -nFE and ∆G = ∆G° + RTlnQ E = E° – RT/nF lnQ 4 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, Ecell (assume volume is 1.0 liter in each compartment) after the two hours have passed. 5 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– Cathode half reaction: Ag(1.0 M) + e– → Ag(s) Overall cell reaction: Ag+(1.0 M) → Ag+(0.01 M) E° = 0.00 volt 6 Calculate Ksp for AgI(s) given the following: Ecell = 0.416 volt for: Ag(s) | Ag+(satd AgI) || Ag+(0.1 M) | Ag(s) Overall cell reaction: Ag(0.1 M) → Ag+(? M) 7 ...
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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_Color - Feeling Stressed? Among the...

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