Workbook Lesson pkt Lesson 13 - Formal Oxidation number assignments - with examples and homework Lesson 28 - Balancing Redox Reactions with examples and homework
Sect (slides provided)
Galvanic Cell schematic Oxidation occurs at anode (vowels) Reduction occurs at cathode (consonants) Oxidation produces electrons, so current flows from anode to cathode.
Types of cells Standard Hydrogen cell platinum electrode metal electrodes
Cell Potential & Nernst Equation Galvanic Cell Potentials - free energy G o = -nFE o F is Faraday constant C/mol e- n = moles of e- from balanced Redox eqn Concentration Cell Potentials G = G o + RTlnQ or K if E cell = 0
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 /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
Equilibrium, K constant E = E o - RT/nF log Q At equilibrium E cell = 0 and Q = K 0 = E o /n log K log K = nE o /