1) Glucose-6P (G6P) has a AGo of approximately -13.8 kJ/mole. Will the transfer of Glu- to ADP to make Glu and ATP be spontaneous or not? (remember the hydrolysis of ATP to ADP and Pi is -30.5 kJ/mole) What is the AG° of that reaction? 2) Pyruvate has three carbons. Draw pyruvate and indicate which carbon is the most oxidized and which is the most reduced. 3) For the written reaction, which reactant is the oxidizing agent, and which is the reducing agent: Co + 2Fe*3 -> Co+2 + 2Fe+2

1) Glucose-6P (G6P) has a AGo of approximately -13.8 kJ/mole. Will the transfer of Glu- to ADP to make Glu and ATP be spontaneous or not? (remember the hydrolysis of ATP to ADP and Pi is -30.5 kJ/mole) What is the AG° of that reaction? 2) Pyruvate has three carbons. Draw pyruvate and indicate which carbon is the most oxidized and which is the most reduced. 3) For the written reaction, which reactant is the oxidizing agent, and which is the reducing agent: Co + 2Fe*3 -> Co+2 + 2Fe+2

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 62E: In glycolysis, the reaction of glucose (Glu) to form glucose-6-phosphate (G6P) requires ATP to be...

See similar textbooks

Similar questions

When glucose, C6H12O11, is metabolized to CO2 and H2O in living systems, the first step is the conversion of glucose to glucose-6-phosphate. glucose+H3PO4glucose-6-phosphate+H2OG=13.4kJ This nonspontaneous reaction can be made to proceed by coupling it with the hydrolysis of ATP. ATP+H2OADP+H3PO4G=31.0kJ (a) Write an equation for the coupled reaction and calculate G°. (b) Estimate the number of moles of ATP required to convert glucose to glucose-6-phosphate.
Consider the following reactions at 25°C: C6H12O6(aq)+6O2(g)6CO2(g)+6H2O G=2870kJ ADP(aq)+HPO42(aq)+2H+(aq)ATP(aq)+H2OG=31kJ Write an equation for a coupled reaction between glucose, C6H12O6, and ADP in which G=390kJ .
Cells use the hydrolysis of adenosine triphosphate (ATP) asa source of energy. The conversion of ATP toADP has a standard free-energy change of -30.5 kJ/mol. Ifall the free energy from the metabolism of glucose, C6H12O6(s) + 6 O2(g)---->6 CO2(g)- + 6 H2O(l) goes into the conversion of ADP to ATP, how many moles ofATP can be produced for each mole of glucose?
What terms would best describe the above coupled reaction? (the DGo for ATP hydrolysis into ADP + inorganic phosphate is -7.3 kcal/mole, and the DGo for sucrose synthesis from glucose + fructose is +5.5 kcal/mole) it is non-spontaneous and endothermic (because the overall DGo is positive) it is spontaneous and exothermic (because the overall DGo is positive) it is non-spontaneous and exothermic (because the overall DGo is positive) it is spontaneous and exothermic (because the overall DGo is negative) it is non-spontaneous and endothermic (because the overall DGo is negative)
How is chemical equilibrium related to transfer of oxygen in blood? How does this relate to the Gibb's Free energy change in oxygen transfer in the tissues? Please answer only the second question.
In glycolysis, the reaction of glucose (Glu) to form glucose-6-phosphate (G6P) requires ATP to be present as described by the following equation:Glu+ATP⟶G6P+ADP ΔG°=−17 kJ In this process, ATP becomes ADP summarized by the following equation:ATP⟶ADP ΔG°=−30 kJ Determine the standard free energy change for the following reaction, and explain why ATP is necessary to drive this process:Glu⟶G6P ΔG°=?
a) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) = -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l) b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?
What is the relationship between free-energy change for a reaction and it's equilibrium constant?
How much free energy would be needed to obtain 7.8 mM of ATP at 37 ° C, if both ADP and inorganic phosphate (Pi) are at 0.3 mM? Please notice that the are asking to make ATP. ADP + Pi + free energy → ATP + H2O The answer should be one of the following: A. +11.5 kJ/mol B. –10.1 kJ/mol C. –8.4 kJ/mol D. –11.5 kJ/mol E. +8.4 kJ/mol Please make sure that the minus/plus on the energy is correct. Please notice that there is a similar answer on the web, but it is not correct.
Would you expect the reaction ATP → ADP + Pito be accompanied by a decrease or increase in entropy? Why?
cells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be written as ATP(aq) + H2O(l)--> ADP(aq) + H2PO4-(aq). where ADP represent adenosine diphosphate. For this reaction, ΔG∘=-30.5kj/mol. a. If all the free energy from the metabolism of glucose goes into forming ATP from ADP, how many ATP molecules can be produced for every molecule of glucose? C6H12O6 + 6O2 → 6CO2 + 6H2O
which of the following has the largest entropy?