Reference no: EM132353134

Consider the reaction M <===> V.  At equilibrium at 37 °C, (M)_eq = 0.1 M and (V)_eq = 10 mM.

What is ΔG'° in kJ/mol for this reaction? answer is 5.9 I've got this

Consider the reaction in the previous question. In the cell, (M) = 10 mM and (V) = 0.1 M.

What is ΔG' in kJ/mol for this reaction?  The answer is 11.9, but I need someone to show me how to work it out

Consider the reaction in the previous questions. If V is fructose 6-phosphate, consider the reaction:

M + H₂O <===> Fructose + P_i  

The equilibrium constant for the last reaction is: answer greater than 1, but I need someone to show me how to work out this question with the provided reaction table.

Reaction ΔG'° (kJ/mol)

Phosphoenolpyruvate + H₂O → Pyruvate + P_i -61.9

1,3-bisphosphoglycerate + H₂O → 3-Phosphoglycerate + P_i -49.3

ATP + H₂O → AMP + PP_i -45.6

Phosphocreatine + H₂O → Creatine + P_i -43.0

ADP + H₂O → AMP + P_i -32.8

Acetyl CoA + H₂O → Acetate + Coenzyme A -31.4

ATP + H₂O → ADP + P_i -30.5

Glucose-1-P + H₂O → Glucose + P_i -20.9

Pyrophosphate (PP_i) + H₂O → 2 P_i -19.2

Fructose-6-P + H₂O → Fructose + Pi -15.9

AMP + H₂O → Adenosine + P_i -14.2

Glucose-6-P + H₂O → Glucose + P_i -13.8

Glycerol-3-P + H₂O → Glycerol + Pi -9.2