The standard reduction potentials for two biologically...

The standard reduction potentials for two biologically relevant redox reactions are as follows: NAD+ + H+ + 2e- ↔ NADH (E°' = -0.315 V) FAD + 2H+ + 2e- ↔ FADH2 (E°' = -0.219 V) What is the standard reduction potential change (ΔE°') for an overall reaction in which NADH is oxidized and the electrons released are used to reduce FAD? 1. -0.534 V 2. -0.096 V 3. +0.096 V 4. +0.534 V

The standard reduction potential, $E^{\prime 0},$ of any redox pair is defined for the half-cell reaction: Oxidizing agent $+n$ electrons $\rightarrow$ reducing agent The $E^{\prime \circ}$ values for the $\mathrm{NAD}^{+} / \mathrm{NADH}$ and pyruvate/lactate conjugate redox pairs are -0.32 V and $-0.19 \mathrm{V},$ respectively. (a) Which redox pair has the greater tendency to lose electrons? Explain. (b) Which pair is the stronger oxidizing agent? Explain. (c) Beginning with $1 \mathrm{M}$ concentrations of each reactant and product at $\mathrm{pH} 7$ and $25^{\circ} \mathrm{C}$ in which direction will the following reaction proceed? $$\text { Pyruvate }+\mathrm{NADH}+\mathrm{H}^{+} \rightleftharpoons \text { lactate }+\mathrm{NAD}^{+}$$ (d) What is the standard free-energy change $\left(\Delta G^{\prime \prime}\right)$ for the conversion of pyruvate to lactate? (c) What is the equilibrium constant $\left(K_{e q}^{\prime}\right)$ for this reaction?

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