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

Please show the calculation in details and in order. Thank you !

Explanation / Answer

1. equilibrium constant = [ glucose-6-phosphate ] / [ glucose-1-phosphate ] = 17.45

free energy = - RT ln K = -7084.8 J/mol

2. actual reduction potential = 0.032 + ln (.111) = -2.166 V

delta G = - n F E = - 2*96500*(-2.166) = 418.0 KJ

3. the free energy of ATP synthesis = -30.5 KJ/mol

So, the delta G will now become -18.5 + 30.5 KJ/mol = +12 KJ/mol

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