jthec
  • jthec
Glycerol 3-phosphate dehydrogenase catalyzes the reversible reaction: G3P + NAD+ --> NADH + H+ + DHAP If in the cell, the concentrations of G3P, NAD+, NADH, and DHAP are 2 mM, 4 mM, 6 mM, and 8 mM respectively. Determine if the reaction spontaneous as written? DHAP + 2e– + 2H+ -->G3P DE'° = –0.29 V NAD+ + H+ + 2e– --> NADH DE'° = –0.32 V
Biology
  • Stacey Warren - Expert brainly.com
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SOLVED
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schrodinger
  • schrodinger
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Frostbite
  • Frostbite
Heya @jthec Do you know how to relate standard reduction potentials to free energy changes?
Frostbite
  • Frostbite
If not I just go over the theory and help you solve the problem from the start.
jthec
  • jthec
I found the overall standard reduction potential difference (-0.03V) and then plugged that into the equation DG = -nFDE

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jthec
  • jthec
But then what do I do with the concentrations? Do I need them?
Frostbite
  • Frostbite
You sure do! :) And now I shall show you why (be patient with me, it takes a little time to write out the math)
jthec
  • jthec
Do I then use the value I got for DG', to plug into the equation DG = DG' + RTln[products]/[reactants]
Frostbite
  • Frostbite
Yes. that is it yes.
jthec
  • jthec
Awesome, thanks
Frostbite
  • Frostbite
Cause the when you calculate the \(\textbf{standard}\) reduction potential difference under the biochemical exception condition you assume: 1) all concentrations to be 1 M 2) the pH to be 7 So by calculating that first you got the standard free energy, but then by adding a correction term you can account for the concentrations as you just said! :)
jthec
  • jthec
Thank-you so much
Frostbite
  • Frostbite
No problem, you really solved it your self, so well done!

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