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Unformatted text preview: 2+ in one liter at equilibrium. Ag + Cu 2+ I C Eq 2 2 ] [ ] [ + + = Ag Cu K How to find E for a cell where concentrations are not 1.0 M Given cell notation: 1. Look up half reactions 2. Calculate E for each halfreaction using Nernst Equation At this point you should write BOTH half reactions as reductions and use the sign listed in the E o table when entering voltages into the equation. 3. Calculate Ecell from: E o meter or cell = E o red or right  E o black or left Example: Find Ecell for: Pt│H 2 (1 atm), 0.0675 M HCl ││ 0.025 M KOH │H 2 (1 atm)│Pt You can also calculate solution concentrations: If Ecell = ─0.015 V, Find the Ag + concentration in the right half cell. Pt│Fe 2+ (0.125 M), Fe 3+ (0.068 M)││ Ag + (? M )│Ag From Appendix C: Ag + + 1e ─ → Ag(s) E o = 0.800 V Fe 3+ + 1e ─ → Fe 2+ E o = 0.771 V...
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 Fall '06
 Paul
 Electrochemistry, ac tan ts, Pr oducts

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