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 + Pi
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 + Pi -61.9
1,3-bisphosphoglycerate + H2O → 3-Phosphoglycerate + Pi -49.3
ATP + H2O → AMP + PPi -45.6
Phosphocreatine + H2O → Creatine + Pi -43.0
ADP + H2O → AMP + Pi -32.8
Acetyl CoA + H2O → Acetate + Coenzyme A -31.4
ATP + H2O → ADP + Pi -30.5
Glucose-1-P + H2O → Glucose + Pi -20.9
Pyrophosphate (PPi) + H2O → 2 Pi -19.2
Fructose-6-P + H2O → Fructose + Pi -15.9
AMP + H2O → Adenosine + Pi -14.2
Glucose-6-P + H2O → Glucose + Pi -13.8
Glycerol-3-P + H2O → Glycerol + Pi -9.2