CH302_031011 - Today Galvanic Cells Spontaneous...

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Principles of Chemistry II © Vanden Bout To d ay Galvanic Cells Spontaneous Electrochemistry Electrolytic Cells “Backwards” Electrochemistry
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Principles of Chemistry II © Vanden Bout Balancing Redox Reactions There is a method (actually several) Learn one (4.10-4.12) Practice (worksheet)
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Principles of Chemistry II © Vanden Bout Electrons have a lower free energy in Zn 2+ (and Cu) than Cu 2+ (and Zn) Zn Cu 2+ 2 e - Zn 2+ Cu Depends on the concentrations!
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Principles of Chemistry II © Vanden Bout Which has the lower Standard Gibb's free energy? A. Zn 2+ (1M) + Cu B. Zn + Cu 2+ (I M) C. They are exactly equal
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Principles of Chemistry II © Vanden Bout A moment to think again about Free Energy and Standard Free Energy G Difference in Free Energy between reactants and product under the current conditions (depends on the concentrations of the reactants and products) The concentration will change until G = 0 Difference in Free Energy between reactants and product under standard conditions standard conditions are 1 M for all aqueous species or 1 atm pressure for all gases
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© Vanden Bout Last time, we look at this idea Use a wire to connect the two sides and have e- fow in an external circuit Zn Cu 2+ 2e - Zn 2+ Cu Problem, one side is getting more positive one side is getting more negative. We need to keep each side neutral
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This note was uploaded on 03/27/2011 for the course CHEM 302 taught by Professor Mccord during the Spring '10 term at University of Texas at Austin.

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CH302_031011 - Today Galvanic Cells Spontaneous...

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