Randy Holmes-Farley
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My Tank Thread
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Good work, everyone. Some of them were perfect!
Here's the answer I hoped for:
Vodka contains ethanol (CH3CH2OH)and vinegar contains acetic acid (CH3CO2H). Acetic acid is already partially metabolized (oxidized) relative to ethanol since it has more oxygen and less hydrogen, so ethanol (vodka) should be the winner since one should get energy at each step of oxidation.
Here's the full answer:
When ethanol is metabolized (oxidized), it is first converted into acetaldehyde (CH3CHO) and then into acetic acid. Then the acetic acid is converted into CO2 and water.
I actually didn't know of the intermediary step from ethanol to acetaldehyde when I wrote the question, and especially not that this step actually takes up energy, not releasing it. But then the step from acetaldehyde to acetic acid gives much more energy. So the net step from ethanol to acetic acid gives off energy to the organism doing it.
Then acetic acid is metabolized to CO2 giving off a huge amount of energy.
Since ethanol gives off energy being converted into acetic acid, it is the winner!
For our purposes, the energy from metabolizing them is:
ethanol: 1,540.4 kilojoules per mole
acetic acid: 1,325.3 kilojoules per mole
Ethanol also weighs less per molecule, and since I asked about weight based comparison, it is even more the winner.
Wikipedia has a nice summary on this page:
Ethanol metabolism - Wikipedia, the free encyclopedia
from it:
Energy Calculations
The reaction from ethanol to carbon dioxide and water is a complex one that proceeds in three steps. Below, the Gibbs Free Energy of Formation for each step is shown with ΔGf values given in the CRC.
Complete Reaction: C2H6O(Ethanol)→C2H4O(Acetaldehyde)→C2H4O2(acetic Acid) →Acetyl-CoA→3H2O+2CO2.
ΔGf = Σ ΔGfp − ΔGfo
Step One: Ethanol: −174.8 kJ/mol
Ethanal(Acetaldehyde): −127.6 kJ/mol
ΔGf1 = −127.6 + 174.8 = 47.2 kJ/mol(Endergonic)
ΣΔGf = 47.2 kJ/mol (Endergonic)
Step Two: Ethanal: −127.6 kJ/mol
Acetic Acid: −389.9 kJ/mol
ΔGf2 = −389.9 + 127.6 = −262.3 kJ/mol (Exergonic)
ΣΔGf = −215.1 kJ/mol (Exergonic)
Step Three: (Because the Gibbs energy is a state function, we can skip the Acetyl-CoA (step 3), for which themodynamic values are not known).
Acetic Acid: −389.9 kJ/mol
3H2O+2CO2: −1 500.1 kJ/mol
ΔGf4 = −1 500 + 389.6 = −1 110.5 kJ/mol (Exergonic)
ΣΔGf = −1 325.3 kJ/mol (Exergonic)
[h=4][/h]
Here's the answer I hoped for:
Vodka contains ethanol (CH3CH2OH)and vinegar contains acetic acid (CH3CO2H). Acetic acid is already partially metabolized (oxidized) relative to ethanol since it has more oxygen and less hydrogen, so ethanol (vodka) should be the winner since one should get energy at each step of oxidation.
Here's the full answer:
When ethanol is metabolized (oxidized), it is first converted into acetaldehyde (CH3CHO) and then into acetic acid. Then the acetic acid is converted into CO2 and water.
I actually didn't know of the intermediary step from ethanol to acetaldehyde when I wrote the question, and especially not that this step actually takes up energy, not releasing it. But then the step from acetaldehyde to acetic acid gives much more energy. So the net step from ethanol to acetic acid gives off energy to the organism doing it.
Then acetic acid is metabolized to CO2 giving off a huge amount of energy.
Since ethanol gives off energy being converted into acetic acid, it is the winner!
For our purposes, the energy from metabolizing them is:
ethanol: 1,540.4 kilojoules per mole
acetic acid: 1,325.3 kilojoules per mole
Ethanol also weighs less per molecule, and since I asked about weight based comparison, it is even more the winner.
Wikipedia has a nice summary on this page:
Ethanol metabolism - Wikipedia, the free encyclopedia
from it:
Energy Calculations
The reaction from ethanol to carbon dioxide and water is a complex one that proceeds in three steps. Below, the Gibbs Free Energy of Formation for each step is shown with ΔGf values given in the CRC.
Complete Reaction: C2H6O(Ethanol)→C2H4O(Acetaldehyde)→C2H4O2(acetic Acid) →Acetyl-CoA→3H2O+2CO2.
ΔGf = Σ ΔGfp − ΔGfo
Step One: Ethanol: −174.8 kJ/mol
Ethanal(Acetaldehyde): −127.6 kJ/mol
ΔGf1 = −127.6 + 174.8 = 47.2 kJ/mol(Endergonic)
ΣΔGf = 47.2 kJ/mol (Endergonic)
Step Two: Ethanal: −127.6 kJ/mol
Acetic Acid: −389.9 kJ/mol
ΔGf2 = −389.9 + 127.6 = −262.3 kJ/mol (Exergonic)
ΣΔGf = −215.1 kJ/mol (Exergonic)
Step Three: (Because the Gibbs energy is a state function, we can skip the Acetyl-CoA (step 3), for which themodynamic values are not known).
Acetic Acid: −389.9 kJ/mol
3H2O+2CO2: −1 500.1 kJ/mol
ΔGf4 = −1 500 + 389.6 = −1 110.5 kJ/mol (Exergonic)
ΣΔGf = −1 325.3 kJ/mol (Exergonic)
[h=4][/h]