CHEM 201 - 11.28.07

CHEM 201 - 11.28.07 - Plug in values to E cell = E cell –...

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CHEM 201 – November 28, 2007 The Nernst Equation E cell = E 0 cell – (RT/nF)lnQ n = number of moles Q = reaction coefficient o E 0 cell = E 0 Red + E 0 Ox – E 0 Reduction of Oxidation o E 0 Ox = -E 0 Red Metallic Cu with Fe(III) to give Cu(II) and Fe(II) o Cu(s)|Cu 2+ ||Fe 2+ , Fe 3+ |Pt anode||cathode o E 0 cell = 0.77V + (-0.34)V = 0.43V o Balance the half equations to get the full equation o
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Unformatted text preview: Plug in values to E cell = E cell – (RT/nF)lnQ to find E cell where Q = [Products]/[Reactants] o Class example E cell = 0.43V – 0.18V = 0.25V Q = K at Equilibrium E = 0 (Dead Battery) o E = E cell – (0.02976)log(K c ) o 0 = 0.43V – (0.0296)log(K c ) o logK = 14.5 K = 3.3x10 14 o...
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This note was uploaded on 04/07/2008 for the course CHEM 201 taught by Professor Harris during the Fall '07 term at Bucknell.

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