Discussion
The relationship between an oxidation-reduction potential difference and the standard free energy change is (where n is the number of moles of electron transferred, F= Faraday's constant and E°= standard oxidation-reduction potential difference)
Answer: A
Correct answer: ΔG° = -nFE°
The relation between redox potential and free energy is
\[ \Delta G^{\circ} = -nFE^{\circ} \]The minus sign is the point: a positive potential difference - electrons falling to a more electropositive acceptor - gives a negative \(\Delta G\), that is a spontaneous, energy-releasing reaction. \(n\) is the number of moles of electrons and \(F\) the Faraday constant, 96.5 kJ per volt per mole.
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