Consider the following reaction at 25 degrees celsius, Pyruvate + Ethanol ---->

Question

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

Standard free energy change for the reaction is -25.1 KJ/mol

Pyruvate + Ethanol ----> Acetalaldehyde + Lactate. this reaction is highly spontaneous.the reaction here is the alcholic fermentation.

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