Please answer the following question including how you arrived to the answer. I
ID: 48122 • Letter: P
Question
Please answer the following question including how you arrived to the answer. I asked this question earlier, and they did not explain how they arrived tot the answer, and didn't answer all my questions.
Consider the following reaction at 25 degrees celsius, Pyruvate + Ethanol ----> Acetalaldehyde + Lactate
a). Using the data from table 10.4, calculate the standard free energy change for the reaction in kJ/mol.
Table 10.4: Standard Gibbs Free energies of hydrolysis for common metabolites:
Metabolite: Delta G hydrolysis (kJ mol ^-1)
Phosphoenolpyruvate -62
1, 3-Bisphosphoglycerate -49
ATP to AMP + PPi -45
Phosphocreatine -43
Phosphoarginine -32
Acetyl CoA -32
Acyl CoA -31
ATP to ADP + Pi -32
Pyrophosphate -29
Glucose 1-phosphate -21
Glucose 6-phosphate -14
Glycerol 3-phosphate -9
b). Is the reaction spontaneous as written?
c). If the concentration of concentrations of ethanol, pyruvate, and lactate are each 1.00 mM, what does the concentration of acetaldehyde need to be to make the reaction spontaneous?
Explanation / Answer
a. Standard free energy change can be calculated using the following equation: ?Go = ?Gof(products) - ?Gof(reactants)
The value obtained from the reaction is -25.1 KJ/mol.
b. Pyruvate + Ethanol ----> Acetalaldehyde + Lactate.
This reaction is highly spontaneous and is a alcholic fermentation reaction.
c. For the reaction to be spontaneous, the concentration of the products should be lower than the concentration of the reactants. Therefore, the concentration of the acetaldehyde need to be lower than 1.00 mM for the reaction to be spontaneous.