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Chem208_Lecture_24_BW

Chem208_Lecture_24_BW - 5 Fe 3 aq Mn 2 aq 4 H 2 O l 5...

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1 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
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2 G = G° + RT ln Q 0 = G ° + RT ln K G ° = –RT ln K Review
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3 Temperature Dependence of K G° = –RT ln K G° = H° - T
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4 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 : 5 Fe 2+ ( aq ) + MnO 4 ( aq ) + 8 H + ( aq ) 5 Fe 3+
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Unformatted text preview: 5 Fe 3+ ( aq ) + Mn 2+ ( aq ) + 4 H 2 O( l ) 5 Consider the reaction: 2 Ag + ( aq ) + Cu ( s ) → 2 Ag ( s ) + Cu 2+ ( aq ) Shorthand Cell Description: Cu (s) | Cu 2+ (aq) || Ag + (aq) | Ag (s) Anode Cathode 6 What is the shorthand version of the cell for 5 Fe 2+ ( aq ) + MnO 4 – ( aq ) + 8 H + ( aq ) → 5 Fe 3+ ( aq ) + Mn 2+ ( aq ) + 4 H 2 O( l ) 7 Relationship between ∆ G and E w elec = 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 8 From thermodynamics, G = -w So, ∆ G = –nFE Under standard conditions: ∆ G° = –nFE°...
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