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Published byMichael Harding Modified over 4 years ago

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Unit 10 - Chpt 18 - Electrochemistry Balance Redox equations HW set1: Chpt 18 - pg. 862-865 # 30, 32 - Due Tues. Apr 20 HW set2: Chpt 18 - pg. 862-865 # 40, 44, 50, 54, 60, 65, 74 - Due Fri. Apr 23

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Workbook Lesson pkt Lesson 13 - Formal Oxidation number assignments - with examples and homework Lesson 28 - Balancing Redox Reactions with examples and homework

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Sect 18.2 - 18.5 (slides provided)

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Galvanic Cell schematic Oxidation occurs at anode (vowels) Reduction occurs at cathode (consonants) Oxidation produces electrons, so current flows from anode to cathode.

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Types of cells Standard Hydrogen cell platinum electrode metal electrodes

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Cell Potential & Nernst Equation Galvanic Cell Potentials - free energy G o = -nFE o F is Faraday constant 96485 C/mol e- n = moles of e- from balanced Redox eqn Concentration Cell Potentials G = G o + RTlnQ or K if E cell = 0

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Cell Potential & Nernst Equation G = G o + RT ln Q -nFE = -nFE o +RT ln Q E = E o - RT/nF ln Q E = E o - 0.0592/n log Q So E of a cell with concentrations not equal to 1 M is the std cell potential with the correction remember to know electrons transferred in Redox

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Equilibrium, K constant E = E o - RT/nF log Q At equilibrium E cell = 0 and Q = K 0 = E o - 0.0592/n log K log K = nE o / 0.0592

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K example Example 18.10 pg 841

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Battery - Dry Cell

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