Alcohol dehydrogenase catalyzes the following reversible reaction:
acetaldehyde + NADH + H⁺

\rightarrow

ethanol + NAD⁺
Use the following information to answer the questions below:
acetaldehyde + 2H⁺ + 2e^-

\rightarrow

ethanol
E'° = -0.20 V
NAD⁺ + H⁺ + 2e^-

\rightarrow

NADH
E'° = -0.32 V
The Faraday constant, $Alcohol dehydrogenase catalyzes the following reversible reaction: acetaldehyde + NADH + H+ \rightarrow ethanol + NAD+ Use the following information to answer the questions below: acetaldehyde + 2H+ + 2e- \rightarrow ethanol E'° = -0.20 V NAD+ + H+ + 2e- \rightarrow NADH E'° = -0.32 V The Faraday constant, , is 96.48 kJ/V · mol. (a) Calculate \Delta G'° for the reaction as written. Show your work. (b) Given your answer to (a), what is the \Delta G'° for the reaction occurring in the reverse direction? (c) Which reaction (forward or reverse) will tend to occur spontaneously under standard conditions? (d) In the cell, the reaction actually proceeds in the direction that has a positive \Delta G'°. Explain how this could be possible.$ , is 96.48 kJ/V · mol.
(a) Calculate

\Delta

G'° for the reaction as written. Show your work.
(b) Given your answer to (a), what is the

\Delta

G'° for the reaction occurring in the reverse direction?
(c) Which reaction (forward or reverse) will tend to occur spontaneously under standard conditions?
(d) In the cell, the reaction actually proceeds in the direction that has a positive

\Delta

G'°. Explain how this could be possible.

Under Cellular Conditions (37°C), What Is the Actual Free Energy ↔\leftrightarrow↔

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Under Cellular Conditions (37°C), What Is the Actual Free Energy $\leftrightarrow$

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