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11 Dec 2019

Given ÎGË' for each of the following reactions: ATP->ADP + Pi ÎGË'= -30.5 kj/mol Glucose-6-phosphate-> glucose + Pi ÎGË'= -13.8 kj/mol Show how you would calculate the standard free energy change (ÎGË') for the overall reaction: ATP + glucose -> glucose-6-phosphate+ ADP Then, How do you calculate the equilibrium constant K'eq for the overall reaction that is above at 25ËC?

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Nestor RutherfordLv2

13 Dec 2019

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Use the free-energy values given below to predict whether the conversionof creatine phosphate to creatine will provide enough energy to phosphorylate ADP. Determine the net reaction and then calculate the overall ÎG⁰'. Is net reaction spontaneous?

Creatine Phosphate + H20 -> Creatine + Pi

ÎG⁰'= -43.1 kJ/mol

ADP + Pi -> ATP + H2O

ÎG⁰'= 30.5 kJ/mol

In the first step of glycolysis, the following two reactions arecoupled:

Reacton 1: glucose + Pi ---> glucose-6-phosphate +H2O Delta G=+13.8 kJ/mol

Reaction 2: ATP + H2O ---> ADP + Pi Delta G=-30.5 kJ/mol

2. Write the net chemical equation. Use the same spelling asshown in the reaction above.

_________________ + ___________________ ----->________________ + ______________________

For the isomerization of glucose-1-phosphate to glucose-6-phosphate, the ÎGÂ°â² = . [Express your answer in kJ/mol using 2 significant figures.]

At 37Â°C and concentrations of 5 mM glucose-6-phosphate and 0.1 mM glucose-1-phosphate, the ÎG = . [Express your answer in kJ/mol using 2 significant figures.]

TABLE12.4Standard Free Energy Change for Phosphate Hydrolysis

COMPOUND

ÎGÂ°^â² (kJ Â· mol^â1)

Phosphoenolpyruvate

â61.9

1,3-Bisphosphoglycerate

â49.4

ATP â AMP + PP_i

â45.6

Phosphocreatine

â43.1

ATP â ADP + P_i

â30.5

Glucose-1-phosphate

â20.9

PP_i â 2 P_i

â19.2

Glucose-6-phosphate

â13.8

Glycerol-3-phosphate

ââ9.2

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