20.2 oxidative Phosphorylation Depends o standard reduction potentials of some r

Question

20.2 oxidative Phosphorylation Depends o standard reduction potentials of some reactions 20.1 1able Reductant dant Eo (N) a-Ketoglutarate -0.67 cinate Acetaldehyde 0.60 (oxidized) Ferredoxin (reduced) doxin -0.43 -0.42 NADH H -0.32 NADPH H+ -0.32 (oxidized) Lipoate (reduced) -0.29 lipoate Glutathione (oxidized) Glutathione (reduced -0.23 -0.22 FADH2 -0.20 Ethanol Acetaldehyde Lactate Pyruvate 0.07 Cytochrome b (+2) Cytochrome b (+3) 0.08 Ascorbate Dehydroascorbate +0.10 Ubiquinone (oxidized) Ubiquinone (reduced) 1 to 22 Cytochrome c (+2) Cytochrome c 3) +0.77 Fe (+2) Fe(+3) -t 0.82 the standard oxidation-reduction potential (pH 25%, except where noted), and n is the number of electrons transferred. Eo refers the partial reaction written as oxidant t e Standard oxidation-reduction potential at pH 0. and has a negative reduction potential, whereas a strong n donate electron accept electrons and has a positive couples a o) is ready to important redox ential The reduction potentials of many biologically chemistry textbooks, ented in

Explanation / Answer

The ions having more the reduction potential, more easily it gets reduced. So, in the table, Fe3+/2+ has reduction potential of 0.77 V, which is quite high. It means that itself gets reduced easily and oxidises another apecie. Reduction means gain of electrons and oxidation is loss of electrons. Fe3+ is gaining an electron and other specie is losing the electron. Suppose Fe3+ is with cytochrome. So, cytochrome will lose an electron to transfer it to Fe3+ which gains the electron to get reduced.

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