Question

From the biological standard half-cell potentials E?(O2,H+,H2O) = +0.82 V and E?(NAD+,H+,NADH) = -0.32 V, calculate the standard potential arising from the reaction in which NADH is oxidized to NAD+ and the corresponding biological standard reaction Gibbs energy.

          From the biological standard half-cell potentials
E?(O2,H+,H2O) = +0.82 V and
E?(NAD+,H+,NADH) = -0.32 V, calculate
the standard potential arising from the reaction
in which NADH is oxidized to NAD+ and the
corresponding biological standard reaction Gibbs
energy.

From the biological standard half-cell potentials
E?(O2,H+,H2O) = +0.82 V and
E?(NAD+,H+,NADH) = -0.32 V, calculate
the standard potential arising from the reaction
in which NADH is oxidized to NAD+ and the
corresponding biological standard reaction Gibbs
energy.

Added by Teresa C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

12/05/2022

Step 1

In this case, the half-reactions are the oxidation of NADH to NAD+ and the reduction of O2 to H2O. The standard potential of the reaction (E°) is given by the equation: E° = E°(O2/H2O) - E°(NAD+/NADH) Substituting the given values: E° = +0.82 V - (-0.32 V) = Show more…

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From the biological standard half-cell potentials E⊕(O2,H+,H2O) = +0.82 V and E⊕(NAD+,H+,NADH) = -0.32 V, calculate the standard potential arising from the reaction in which NADH is oxidized to NAD+ and the corresponding biological standard reaction Gibbs energy.