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Unformatted text preview: 1 Electron Transport and Oxidative Phosphorylation Chapter 13 (512-521) Chapter 19 (707-741) 16-1 Electron transport = transfer of e- from one carrier to another Oxidative phosphorylation = process by which energy released from electron transport (oxidations) is conserved in form of phosphate-bond energy of ATP Oxidation-reduction reactions = transfer of electrons from a donor (reducing agent) to an acceptor (oxidizing agent). Analogous to acid-base reaction: acid/base: proton acceptor + H + proton donor redox: electron acceptor + e- electron donor Tendency of a substance to give up electrons (to be oxidized) is reflected in the standard reduction potential , E° A o + e- A r E° A B o + e- B r E° B A o + B r A r + B o ∆ E° = E° A- E° B = reduction potential difference (acceptor) (donor) 13-23 H + + e- 1/2H 2 E° = 0.0 V (standard conditions) oxidant + n e- reductant n = # electrons transferred The more negative the potential for a redox pair, reductant has greater tendency to lose electrons. More positive, reductant has less tendency to lose electrons. ∆ E°' is related to ∆ G°' and K eq by: = − nF ( E ° ' acceptor − E ° ' donor ) Δ G ° ' = − nF Δ E ° ' F = Faraday constant = 96494 coulomb/mol = J/volt•mol n = # mol electrons transferred Rearrange: Δ E ° ' = − Δ G ° ' nF = RT nF ln k eq 2...
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This note was uploaded on 05/04/2010 for the course CH 53890 taught by Professor Raymonds during the Spring '09 term at University of Texas at Austin.
- Spring '09