1.Under Standard conditions, equilibrium concentrations are 9.6x10^-2M glucose-6

Question

1.Under Standard conditions, equilibrium concentrations are 9.6x10^-2M glucose-6-phosphate and 5.5x10^-3M glucose-1-phosphate. What is the delta G for the conversion of glucose-1-phosphate into glucose-6-phosphate? Show your work.

2. Consider the following reaction: fumarate + 2H^+ + 2e- -> succinate

a. What is the actual reduction potential of fumarate assuming that delta E' * = +0.032 V [fumarate] =1M, and [succinate] = 0.111M

b. What is the actual delta G for this reaction

3.Consider this reaction: 1,3-bisphosphoglycerate + ADP ---> 3-phosphoglycerate + ATP. The delta G'* of this coupled reaction is -18.5 k/mol. What is the delta G'* of the reaction if ATP is not synthesized? Show the work

Explanation / Answer

1.First calculate the equilibrium constant by using the Gibbs' relation:

G = -RTln(K)

deltaG = deltaG^o + R*T*ln ([F6P]/[G6P])

Now that you know the value of K you can determine the equilibrium concentrations by writing the equilibrium equation:

1) For any reaction, the relationship between Keq and ?G

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