Chem208_Lecture_24_Color - Today: Finish Thermodynamics...

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Unformatted text preview: Today: Finish Thermodynamics (Ch. 19) - T dependence of K (19-7) Start Electrochemistry (Ch. 20) - Galvanic Cells (20-1/6) PS9 is due Friday, 4/18, at 2:00 (tomorrow) Pick up or download PS10 today; Due Friday, 4/25, at 2:00 1 Review ∆G = ∆G° + RTlnQ 0 = ∆G° + RTlnK ∆G° = –RTlnK 2 Temperature Dependence of K ∆G° = –RTlnK ∆G° = ∆H° - T∆S° 3 Chem 207 Review • Oxidation: loss of electrons or increase in oxidation state • Reduction: gain of electrons or decrease in oxidation state • Oxidizing Agent: the species that oxidizes another species, and gets reduced in the process • Reducing Agent: the species that reduces another species, and gets oxidized in the process Example: 4 2+(aq) + MnO –(aq) + 8 H+(aq) → 5 Fe3+(aq) + Mn2+(aq) + 4 H O(l) 5 Fe 4 2 Consider the reaction: 2 Ag+ (aq) + Cu (s) → 2 Ag(s) + Cu2+(aq) Shorthand Cell Description: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Anode Cathode 5 What is the shorthand version of the cell for 5 Fe2+(aq) + MnO4–(aq) + 8 H+(aq) → 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(l) 6 Relationship between ∆G and E welec = nFE (work done by the system) n: # of moles of electrons transferred F: charge on 1 mole of electrons (the Faraday) (F = 96,485 coulombs) E: cell potential 7 From thermodynamics, G = -w So, ∆G = –nFE Under standard conditions: ∆G° = –nFE° 8 ...
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Chem208_Lecture_24_Color - Today: Finish Thermodynamics...

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