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Unformatted text preview: 2 (s) + 2H + + 2e- Ni(OH) 2 (s) Cd(s) + 2H 2 O + NiO 2 (s) Cd(OH) 2 + Ni(OH) 2 In the Cu cell In the Zn cell Cu Cu 2+ Zn 2+ Zn Cu 2+ Cu Zn Zn 2+ (one of these two (one of these two things must be things must be happening) happening) use the reduction potentials to figure out which one of these cells is the oxidation (anode) and which is the reduction (cathode) Standard Reduction Potentials are: Cu 2+ + 2e- Cu E o = +0.332 v Zn 2+ + 2e- Zn E o = -0.763 v two possibilities. 1. Oxid. Cu Cu 2+ + 2e-E o = -0.337 v Red. Zn 2+ + e- Zn. E o = -0.763 v Cu + Zn 2+ Cu 2+ + Zn E o = -1.10 2. Oxid. Zn Zn 2+ + 2e-E o = +0.763 v Red. Cu 2+ + 2e- Cu E o = +0.337 v Zn + Cu 2+ Zn 2+ + Cu E o = +1.10 v possibility #2 is the reaction that occurs spontaneously since E o is +. possibility #1 possibility #2...
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This note was uploaded on 12/02/2011 for the course PHYSICS 235 taught by Professor Staff during the Fall '08 term at Rutgers.
- Fall '08