Consider the oxidation of ethanol by NAD+ to from acetaldehyde: NAD++C2H5OH?NADH

Question

Consider the oxidation of ethanol by NAD+ to from acetaldehyde: NAD++C2H5OH?NADH+CH3CHO+H+ Assuming standard half-cell reduction potentials: E0’NAD+/NADH=-0.32 V and E0’CH3CHO/EtOH=-0.18V calculate the standard cell potential E0’, the standard Gibbs energy change ?G°’, and the equilibrium constant K’. Based on your answer, does the system favor the formation of acetaldehyde or ethanol at equilibrium? T=320K. Please explain how you got to the answer that you did. The way that I approached this question is by adding the half cell reduction potentials, and then using deltaGprime=-nFE, but I'm not entirely sure how to find n.....

Explanation / Answer

Given

Eo red E0’NAD+/NADH=-0.32 V

Eo ox E0’CH3CHO/EtOH=-0.18V

Eo cell =Eo oxidation + Eo reduction.

              (-0.18) +(-0.32)

= -0.5 V

Hence tandard cell potential E0 = -0.5 V

G°cell = nFE°cell.

n=number of mole of electron

F= Faradays constant= 96,485Coulombsmole

G°cell = -1 x 96,485 x -0.5 =48242 joules= 48.24kJ

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