standard free energy change for the following reaction: ATP+H₂O-ADP PL. Which two of the following statements are the correct reasons for the reaction to have such a large negative AG" value? 1. decrease in electrostatic repulsion by the cleavage of phosphoanhydride bond. 2. decrease in electrostatic repulsion by the cleavage of phosphoester bond. 3. more resonance stabilization in ATP than in Pi 4. more resonance stabilization in Pi than in ATP

standard free energy change for the following reaction: ATP+H₂O-ADP PL. Which two of the following statements are the correct reasons for the reaction to have such a large negative AG" value? 1. decrease in electrostatic repulsion by the cleavage of phosphoanhydride bond. 2. decrease in electrostatic repulsion by the cleavage of phosphoester bond. 3. more resonance stabilization in ATP than in Pi 4. more resonance stabilization in Pi than in ATP

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...

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Which of the reactions are spontaneous (favorable)? DHAP = glyceraldehyde-3-phosphate AG = 3.8 kJ/mol L-malate + NAD+ → oxaloacetate + NADH + H+ AG = 29.7 kJ/mol C,H¸O; C,H,O, + H,0 AG= 3.1 kJ/mol Rh(I) C,H, + H, C,H, AG = -150.97 kJ/mol C,H1,0,P O̟P + ATP C,H14012P2 + ADP AG = -14.2 kJ/mol glutamate + NAD+ + H,O → NH† + a-ketoglutarate + NADH + H* AG = 3.7 kcal/mol
Although the ATP-ADP reaction is the principle energy shuttle in metabolic pathways, many other examples of coupled reactions exist. glutamic acid + NH3 glutamine + H2O, ΔGo = 14 kJ. Can be coupled with the acetyl phosphate reaction shown CH3COOPO3H2 + H2O CH3COOH + H3PO4, ΔGo = -46.9 kJ a. Calculate ΔGo for the overall process.
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The reaction converting glycerol to glycerol-3-phosphate is energetically unfavorable by 9.2 kJ. The reaction of ATP with water to yield ADP, hydrogen phosphate ion, and hydrogen ion is energetically favorable by 30.5 kJ. These reactions are coupled so that the overall process is energetically favorable. What is AG for the overall process? Express your answer with the appropriate units. View Available Hint(s) ? HA AG = Value Units
Hydrolysis of ATP is favorable (AGo' = = -30.5 kJ/mol), but the addition of inorganic phosphate (Pi) to glucose to yield glucose-6-phosphate, the first step in glycolysis, is unfavorable (AGo' = +13.8 kJ/mol). Show how these two reactions can be coupled to favor formation of glucose-6-phosphate and allow glycolysis to proceed. Include the overall AGo' for the reaction.
Consider 2 reactions, for which the standard free energy changes are given: Reaction 1: Glucose-1-phosphate + UTP --> UDP-glucose + pyrophosphate AG° = ~0 kJ/mol Reaction 2: pyrophosphate --> 2 Pi AG = -19.2 kJ/mol Which statement is CORRECT concerning these 2 reactions? A reaction that couples reaction 1 and 2 together is not feasible. O A reaction that couples reaction 1 and 2 together would be very slow. A reaction that couples reaction 1 and 2 together is thermodynamically favorable. O A reaction that couples reaction 1 and 2 together is kinetically fast.
Which of the reactions are spontaneous (favorable)? 1)DHAP↽−−⇀glyceraldehyde-3-phosphateΔ?=3.8 kJ/mol 2)L-malate+NAD+⟶oxaloacetate+NADH+H+Δ?=29.7 kJ/mol- 3) glutamate+NAD++H2O⟶NH+4+α-ketoglutarate+NADH+H+Δ?=3.7 kcal/ 4) C6H13O9P+ATP⟶C6H14O12P2+ADPΔ?=−14.2KJ/mol 5) −Rh(I)C2H6Δ?=−150.97 kJ/molC2H4+H2→Rh(I)C2H6ΔG=−150.97 kJ/mol 6) C4H4O5⟶C4H2O4+H2OΔ?=3.1 kJ/mol
Chemistry 4.3 Calculate the standard free-energy for creatine-phosphate hydrolysis in a cell where: creatine-P= 60mmol, creatine - 30 mmol, ATP - 1 mmol, ADP-0.1 mmol. Is this reaction exer/endergonic?
Hi, Please help me answer these two questions. Hope I'd get all the items done. PS. If possible, provide explanations on it. Thank you so much. *** 1. Calculate the value of ΔGo’ for the following reaction. Glucose-1-phosphate → Glucose-6-phosphate Given: Glucose-1-phosphate → Glucose + Pi ΔGo’ = -20.9 kJ/mol Glucose + Pi → Glucose-6-phosphate ΔGo’ = +12.5 kJ/mol 2. The ΔGo’ for Coupled Reactions. Glucose-1-phosphate is converted into fructose-6-phosphate in two successive reactions: Glucose 1-phosphate →glucose 6-phosphate ΔGo’ = -7.3 kJ/mol Glucose 6-phosphate→fructose 6-phosphate ΔGo’ = + 1.7 kJ/mol Calculate the overall ΔGo’ and the equilibrium constant, K’eq for the sum of the two reactions: Glucose 1-phosphate → fructose 6-phosphate
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The reaction for “activation” of a fatty acid (RCOO−), ATP + CoA + RCOO−⇌ RCOOCoA + AMP + PPi has ΔG°′ = +4.6 kJ · mol−1. What is the thermo dynamic driving force for this reaction?