The formation of maltose, a disaccharide, from two glucose molecules, is not energetically favorable. However, if this reaction is coupled with the hydrolysis of ATP, the reaction occurs more favorably. Maltose + H2O = 2 Glucose , ΔG'o = -15.5 KJ/mol or -3.7 kcal/mol a. Determine if the coupled reaction will occur spontaneously at standard state through calculating the Gibbs Free Energy of Reaction. b. Calculate the equilibrium constant for each individual reaction, and for the coupled reaction (using free energy of reaction). Show that the equilibrium constant for the coupled reaction equals the equilibrium constants for the individual reactions multiplied together. c. If the reaction medium contains the following chemical species at their given concentrations (298 K and 1.0 atm, pH = 7.0), will the reaction proceed in the forward or the reverse direction? [Maltose] = [Glucose] = 10.0 mM; [ATP] = 5.0 mM; [ADP] = [Pi] = 20 mM
The formation of maltose, a disaccharide, from two glucose molecules, is not energetically favorable. However, if this reaction is coupled with the hydrolysis of ATP, the reaction occurs more favorably.
Maltose + H2O = 2 Glucose , ΔG'o = -15.5 KJ/mol or -3.7 kcal/mol
a. Determine if the coupled reaction will occur spontaneously at standard state through calculating the Gibbs Free Energy of Reaction.
b. Calculate the equilibrium constant for each individual reaction, and for the coupled reaction (using free energy of reaction). Show that the equilibrium constant for the coupled reaction equals the equilibrium constants for the individual reactions multiplied together.
c. If the reaction medium contains the following chemical species at their given concentrations (298 K and 1.0 atm, pH = 7.0), will the reaction proceed in the forward or the reverse direction? [Maltose] = [Glucose] = 10.0 mM; [ATP] = 5.0 mM; [ADP] = [Pi] = 20 mM
The formation of maltose, a disaccharide, from two glucose molecules, is not energetically favorable. However, if this reaction is coupled with the hydrolysis of ATP, the reaction occurs more favorably.
Maltose + H2O = 2 Glucose , ΔG'o = -15.5 KJ/mol or -3.7 kcal/mol
a. Determine if the coupled reaction will occur spontaneously at standard state through calculating the Gibbs Free Energy of Reaction.
b. Calculate the equilibrium constant for each individual reaction, and for the coupled reaction (using free energy of reaction). Show that the equilibrium constant for the coupled reaction equals the equilibrium constants for the individual reactions multiplied together.
c. If the reaction medium contains the following chemical species at their given concentrations (298 K and 1.0 atm, pH = 7.0), will the reaction proceed in the forward or the reverse direction? [Maltose] = [Glucose] = 10.0 mM; [ATP] = 5.0 mM; [ADP] = [Pi] = 20 mM
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