The enzyme aldolase catalyzes the conversion of fructose-1,6-diphosphate (FDP)to dihydroxyacetone phosphate (DHAP) and glyceraldehyde-3-phosphate (G3P). Thereaction isFDP → DHAP + G3PwithA,G°(298.15 K) = 23.8 kJ molIn red blood cells, the concentrations of these species are [FDP] = 35 µM, [DHAP] =%3D130 µM, and [G3P] = 15 µM. Remember that 1.0 µM1.0 x 10-6 mol L-1. Thestandard state for reactions in solution can be taken to be 1.0 mol L-1.(a) Calculate A,G in a red blood cell at 25°C. (Note: A,G is not the same asA,Gº, as the substances in the blood cell are not in standard condi-tions).(b) Will the reaction occur spontaneously in the blood cell at this temperature?

Given that, the enzyme aldose catalyzes the conversion of fructose-1,6-diphosphate (FDP) to…

The enzyme aldolase catalyzes the conversion of fructose-1,6-diphosphate (FDP) to dihydroxyacetone phosphate (DHAP) and glyceraldehyde-3-phosphate (G3P). The reaction is with 4,G°(298.15 K) = 23.8 kJ mol- FDP → DHAP + G3P In red blood cells, the concentrations of these species are [FDP] = 35 µM, [DHAP] = 130 µM, and [G3P] = 15„M. Remember that 1.0 µM = 1.0 × 10-6 mol L-!. The standard state for reactions in solution can be taken to be 1.0 mol L-!. (a) Calculate A,G in a red blood cell at 25°C. (Note: A,G is not the same as A,Gº, as the substances in the blood cell are not in standard condi- tions). (b) Will the reaction occur spontaneously in the blood cell at this temperature?

The enzyme aldolase catalyzes the conversion of fructose-1,6-diphosphate (FDP) to dihydroxyacetone phosphate (DHAP) and glyceraldehyde-3-phosphate (G3P). The reaction is with 4,G°(298.15 K) = 23.8 kJ mol- FDP → DHAP + G3P In red blood cells, the concentrations of these species are [FDP] = 35 µM, [DHAP] = 130 µM, and [G3P] = 15„M. Remember that 1.0 µM = 1.0 × 10-6 mol L-!. The standard state for reactions in solution can be taken to be 1.0 mol L-!. (a) Calculate A,G in a red blood cell at 25°C. (Note: A,G is not the same as A,Gº, as the substances in the blood cell are not in standard condi- tions). (b) Will the reaction occur spontaneously in the blood cell at this temperature?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter23: Organic Polymers, Natural And Synthetic

Section: Chapter Questions

Problem 46QAP: Glycolysis is the process by which glucose is metabolized to lactic acid according to the equation...

See similar textbooks

Similar questions

The standard free energy variation, at 25 ºC, for equilibrium: Glucose-6-phosphate (G-6-P) Glucose-1-phosphate (G-1-P) is ΔGº '= + 7280 J / mol. Calculate a) The equilibrium constant of the reaction. b) The real change in free energy when one mole of G-6-P is transformed into G-1-P, both concentrations remaining constant and equal to 10mM and 2 mM respectively.
Calculate the equilibrium constant at 37oC for the reactionGlucose + 6O2 + 36ADP + 36Phospate → 6CO2+ 42H2O +36ATP ... ... ...Entropy change of Go= − 423 kcal/mole of Glucose
In glycolysis, glucose is broken down to yield energy. If the equilibrium constant of the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.5, would this reaction proceed in the forward or reverse direction? What is the free energy of the reaction? Using standard conditions (1 M) as an initial state, what are the equilibrium concentrations?
For the triose phosphate catalyzed reaction: dihydroxyacetone phosphate <--> glyceraldehyde-3-phosphate the standard change in Gibbs free energy is ΔG'º=7.53 kJ/mol. Calculate the ΔG for this reaction at 298K when the concentration of dihydroxyacetone phosphate is 0.161 M and the concentration of glyceraldehyde-3-phosphate is 0.00163 M.
In liver cells the usual concentrations of some solutes are: [ATP] = 3.4 mM; [ADP] = 1.3 mM and [Pi] = 5 mM. Calculate the real variation of energy free by hydrolyzing ATP in the liver into ADP and Pi. a) at 25ºC b) at 37ºC (ΔGº’ ATP hydrolysis = -30.5 kJ / mol)
In glycolysis, the hydrolysis of ATP to ADP is used to drive the phosphorylation of glucose (GLC): GLC+ATP <--> ADP+GLC-6-phosphat ΔG° = −17.7 kJ What is the value of Kc for this reaction at 298K?
Aerobic respiration links the oxidation of glucose with the production of ATP form ADP.Given the following thermodynamic data, C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔrH° = −2803 kJ/mol-rxn ATP + H2O(l) → ADP + HPO42-(aq) ΔrH° ≈ −24 kJ/mol-rxn calculate the enthalpy of reaction for the aerobic production of 25 ATP shown below.C6H12O6(s) + 6O2(g) + 25ADP + 25HPO42-(aq)→ 6CO2(g) + 25ATP + 31H2O(l) ΔrH° = ?
Calculate the equilibrium constant at 37oC for the reactionGlucose + 6O2 + 36ADP + 36Phospate → 6CO2+ 42H2O +36ATP ... ... ...Gibbs free energychange of Go= − 423 kcal/mole of Glucose
Use the standard reaction energies given below to determine DeltaG^°rxn for the following reaction: 2XO2(g) —> 2XO(g) + O2(g) From the standard reaction energy of X2(g) + O2 —> 2XO(g) DG^°= 155.52 Kjxmol-1 X2(g) + 2O2 —> 2XO2(g) DG^°= 168.55 Kjxmol-1 Given answer in Kj/mol. Give answer to two decimal places.
The standard free energy change for the reaction catalyzed by phosphoglucomutase is -7.1kJ/mol, (a) Calculate the equilibrium constant for the reaction, (b) Calculate ΔG at 37°C when the concentration of glucose-1-phosphate is 1-mM and the concentration of glucose-6-phosphate is 25-mM, (c) Is the reaction spontaneous under these conditions?
What is free energy ∆G° for the reaction C(s) + O₂(g)⇌ CO₂(g) (K= 0.2 at 25°C)?
Consider the reaction CO (g) + 2 H2 (g) = CH3OH (l)Thermodynamic Quantities for Substances at 25°C delta H°f (kJ/mol) delta G°f (kJ/mol) S°(J/mol*K) CO (g) -110.5 -137.2 197.5 H2 (g) 0 0 130.6 CH3OH -201.2 -161.9 238 17(a) Use the data above to calculate deltaH° and delta S° at 25°C. (17b) What is K at 25°C? (17c) What is delta G° at 1000°C?