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Unformatted text preview: Chemistry 102 04/24/08 1. The standard cell potential, E ° (cell), for the reaction of silver ions with copper metal is + .46 V at 25 ° C. Calculate ∆ G ° for this reaction. Cu^2+(aq) + 2e- Cu(s) E ° = +.34 Anode (-) (Oxidation) Ag^+(aq) + e- Ag(s) E ° = .80 Cathode (+) (Reduction) Ox: Cu(s) Cu^2+(aq) + 2e- Red: Ag^+(aq) + e- Ag(s) x2 Cu(s) + 2Ag(aq) Cu^2+(aq) + 2Ag(s) Cu: Anode oxidized Ag: Cathode reduced E ° (cell) = E ° (cathode) - E ° (anode) = .80V – (.34V) = .46 ∆ G ° = -nFT ; F= 96500 C/mol e- n=2 because there are 2e- transferred ∆ G ° = -(2 mol e-) (96,500 C/mol e-) (+.46V)-89,200 C*V = -89.2 KJ Spontaneous 2. Which of the following metals will react with H+(aq) to produce H2 in a product-favored reaction: Cu,Al,Ag,Fe,Zn? Cu^2+ + 2e- Cu(s) E ° = .34V Al^3+ + 3e- Al(s) E ° = -1.66 V Ag+(aq) + e- Ag(s) E ° = .80V Fe^2+(aq) + 2e- Fe(s) E ° = -.44 V Zn^2+ + 2e- Zn(s) E ° = -.76V 3. A voltaic cell is set up at 253....
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This note was uploaded on 04/27/2008 for the course CHEM 112 taught by Professor Seancollins(ta) during the Spring '08 term at Texas A&M.
- Spring '08