Question

Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy ΔG∘: reaction A:reaction B:glucose-1-phosphatefructose-6-phosphate⟶⟶glucose-6-phosphate,glucose-6-phosphate,   ΔG∘=−7.28 kJ/mol   ΔG∘=−1.67 kJ/mol

Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy ΔG reaction A: glucose-1-phosphate .→ glucose-6-phosphate, ΔGo=-7.28 kJ/mol reaction B: fructose-6-phosphate-, glucose-6-phosphate, ΔGn-_1.67 kJ/mol

Part A

Calculate ΔG∘ for the isomerization of glucose-1-phosphate to fructose-6-phosphate.

ΔG∘ =

-5.61

kJ/mol

Part B

Calculate the equilibrium constant K for the isomerization of glucose-1-phosphate to fructose-6-phosphate at 298 K.

Express your answer numerically using two significant figures.

K =

9.6

Part C

Calculate  ΔG when the concentration of glucose-1-phosphate is   10 times greater than the concentration of fructose-6-phosphate.

Please help with Part C: calculate deltaG when [glucose-1-phosphate] is 10 times greater than [fructose-6-phosphate]

Answer 1