Lect+26+08 - Objectives for Electrochemistry Lecture 26 A...

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Objectives for Electrochemistry Lecture 26 A common language understanding of the Nernst Equation Using the Nernst Equation to evaluate Cell Potentials Disproportionation Reactions A common language understanding of pH electrodes A common language understanding of primary and rechargeable batteries Rate laws first order second order homogeneous reversible first order
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When making cell from half cells number of electron must cancel Add the potential of the half cells which make up the cell keeping in mind that the reaction which is being oxidized is running backward and the sign of the reduction potential must be changed 2200 ° (cell) = ° (cathode) - ° (anode)
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The Nernst Equation comes from the Gibbs free energy equation 2200 G = G ° + RT ln Q (from chapter 14) and 2200 G = -n F   and G ° = -n F   ° So substituting in for G and G ° - n F    = - n F    ° + RT ln Q 2200 = ° - {RT / n F    } (ln Q) But ln Q = 2.303 log 10 Q 2200 = ° - 0.0592 V/n (log 10 Q) n is the # of electrons
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Nernst Equation 2200 = ° - 0.0592 V/n (log 10 Q) The voltage of an electrochemical cell depends on the standard potential corrected by a constant times the logarithm of the reaction quotient
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