Electron Transport and Oxidative Phosphorylation
Electron Transport and Oxidative Phosphorylation
Electron Transport and Oxidative Phosphorylation
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Garrett <strong>and</strong> Grisham, Biochemistry, Third Edition<br />
20.2 – What Are Reduction Potentials, <strong>and</strong><br />
How Are They Used to Account for Free<br />
Energy Changes in Redox Reactions?<br />
High E o ' indicates a strong tendency to be reduced<br />
• Crucial equation: ∆G o ' = -nF∆E o '<br />
∆E o ' = E o '(acceptor) - E o '(donor)<br />
• <strong>Electron</strong>s are donated by the half reaction with<br />
the more negative reduction potential <strong>and</strong> are<br />
accepted by the reaction with the more positive<br />
reduction potential: ∆E o ' positive, ∆G o ' negative<br />
• If a given reaction is written so the reverse is true,<br />
then the ∆E o ' will be a negative number <strong>and</strong> ∆G o '<br />
will be positive