5b) Oxidation of lactate to pyruvate by cytochrome C (representing as cytochrome C(Fe"))is an important biolagical reaction. The followings are reduction reactions and the relevantstandart reduction potentials (E°) at pH = 7 and 25°C.Pyruvate + 2H* + 2e° → Lactate"E° = -0,185 VCytochrome Č (Fe") + e° → Cytochrome C (Fe²")E° = 0.254 Vi) Write anodic, cathodic and total reactions.ii) Using the Gibss free energy and Nernst equations calculate the following equilibriumratio (K) at pH=7 and 25°C;[Cytochrome C(Fe²*)]²[Pyruvate][H*]²[Cytochrome C(Fe3+)]²[Lactate¬]

Given Pyruvate + 2H+ + 2e- →Lactate-…

5b) Óxidation of lactate to pyruvate by cytochrome C (representing as cytochrome C(Fe³)) is an important biolagical reaction. The followings are reduction reactions and the relevant standart reduction potentials (Eº) at pH = 7 and 25°C. Pyruvate + 2H' + 2e° → Lactate" E° = -0,185 V Cytochrome C (Fe³") + e ° →Cytochrome C (Fe²") E° = 0.254 V i) Write anodic, cathodic and total reactions. ii) Using the Gibss free energy and Nernst equations calculate the following equilibrium ratio (K) at pH=7 and 25°C;

5b) Óxidation of lactate to pyruvate by cytochrome C (representing as cytochrome C(Fe³)) is an important biolagical reaction. The followings are reduction reactions and the relevant standart reduction potentials (Eº) at pH = 7 and 25°C. Pyruvate + 2H' + 2e° → Lactate" E° = -0,185 V Cytochrome C (Fe³") + e ° →Cytochrome C (Fe²") E° = 0.254 V i) Write anodic, cathodic and total reactions. ii) Using the Gibss free energy and Nernst equations calculate the following equilibrium ratio (K) at pH=7 and 25°C;

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 74QAP: Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to...

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For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
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From the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.
Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
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Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 2.00 with all other ionic species at 0.100 M? (c) Is the reaction spontaneous at a pH of 5.00 with all other ionic species at 0.100 M? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M?
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