Chem notes 4/13 (read 18.6-18.9 ; do 73, 63, 87, 89, 99)Oxidizing and reducing agentsoxidizing agent– acts in the cause of oxidation- causes another species to be oxidized- wants electrons- it is reduced in the rxnreducing agent– acts in the cause of reduction- causes another species to be reduced- gives up electrons- it is oxidized in the rxnThe Nernst Equation- gives the cell voltage when the reagents are not in standard statesrecall ΔG = ΔG° + RTlnQΔG° = - nFΔE° ΔG = - nFΔEsubstitute:- nFΔE = - nFΔE° + RTlnQΔE = ΔE° - (RT/nF) lnQconvert to log base 10ΔE = ΔE° - (2.303 RT/nF) logQΔE = ΔE° - (0.0592V/nF) logQSo, if species are not in their standard states (i.e. concentrations are not 1.00 M) the cell voltage is modified- calculate Q, ΔE°, then calculate ΔE
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