(a)
Interpretation:
The given reaction should be identified that whether it is exergonic or endergonic and also that at equilibrium which side proceeds farthest toward products.
Concept Introduction:
Exergonic: The reaction is considered as exergonic if energy released since the reactants loses its energy making the free energy more negative hence making it spontaneous reaction.
Endergonic: The reaction is considered as endergonic if it needs more energy means that activation energy is much higher making the reaction non spontaneous.
Favorable Reaction: They release free energy which in turn used to do work. The products will have lower energy than reactants of the reaction shows that stable products are obtained hence the value of
The tendency for reaction proceed toward product side before reaching equilibrium will increases as more amount of free energy released.
(b)
Interpretation:
The given reaction should be identified that whether it is exergonic or endergonic and also that at equilibrium which side proceeds farthest toward products.
Concept Introduction:
Exergonic: The reaction is considered as exergonic if energy released since the reactants loses its energy making the free energy more negative hence making it spontaneous reaction.
Endergonic: The reaction is considered as endergonic if it needs more energy means that activation energy is much higher making the reaction non spontaneous.
Favorable Reaction: They release free energy which in turn used to do work. The products will have lower energy than reactants of the reaction shows that stable products are obtained hence the value of
The tendency for reaction proceed toward product side before reaching equilibrium will increases as more amount of free energy released.
(c)
Interpretation:
The given reaction should be identified that whether it is exergonic or endergonic and also that at equilibrium which side proceeds farthest toward products.
Concept Introduction:
Exergonic: The reaction is considered as exergonic if energy released since the reactants loses its energy making the free energy more negative hence making it spontaneous reaction.
Endergonic: The reaction is considered as endergonic if it needs more energy means that activation energy is much higher making the reaction non spontaneous.
Favorable Reaction: They release free energy which in turn used to do work. The products will have lower energy than reactants of the reaction shows that stable products are obtained hence the value of
The tendency for reaction proceed toward product side before reaching equilibrium will increases as more amount of free energy released.
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Fundamentals of General, Organic, and Biological Chemistry (8th Edition)
- In a major metabolic pathway involving the monosaccharide glucose, one of the reactions involve the conversion of glucose to glucose-6-phosphate summarized below together with accompanying free energy change: glucose + phosphate = glucose-6-phosphate + H,0 AG = 13.8 kJ · mol-1 (Reaction 1) In cells, the production of G6P (Reaction 1 above) is coupled to a reaction that involves the hydrolysis of ATP to ADP (shown below, Reaction 2) which makes the overall reaction much more favorable to the production of glucose-6-phosphate. ATP + H,O = ADP + phosphate (Reaction 2) Why do you think coupling the production of glucose-6-phosphate to the hydrolysis of ATP makes the overall reaction spontaneous? What can you say about the free energy change accompanying the hydrolysis of ATP (Reaction 2)?arrow_forwardDuring glycolysis, glucose is converted into fructose-6- phosphate in two successive reactions: glucose + ATP glucose 6-phosphate + ADP glucose 6-phosphate fructose 6-phosphate The AG' for the overall reaction is: +15.0 kJ/mol. -18.4 kJ/mol. -16.7 kJ/mol. → -15.0 kJ/mol. +18.4 kJ/mol. AG¹⁰ = -16.7 kJ/mol AG¹⁰ = +1.7 kJ/molarrow_forwarda) The following reaction which is catalyzed by aldolase: Fructose-,6-bisphosphate (FBP) + Glyceraldehyde 3-phosphate (GAP) + Dihydroxyacetone phosphate (DHAP) AG for this reaction is 22.8 kJ mol'. In the cell at 37°C, AG for this reaction is -5.9 kJ mol". Determine the ratio [GAP][DHAP]/[FBP]arrow_forward
- Assume that you have a solution of 0.1 M glucose 6-phosphate. To this solution you add the enzyme phosphoglucomutase, which catalyzes the reaction: glucose-6-P ⇔ glucose-1-P ∆G°′ = +1.7 kJ/mol (a) Does this reaction proceed at all as written at 25 °C, and if so, what are the final concentrations of glucose 6-P and glucose 1-P? (b) What effect would omitting the enzyme have on the reaction. Be specific. (c) Under what cellular conditions, if any, would this reaction continuously produce glucose 1-P at a high rate?arrow_forwardWhat terms would best describe the above coupled reaction? (If the DGo for ATP hydrolysis into ADP + inorganic phosphate is -7.3 kcal/mole, and the DGo for maltose synthesis from glucose + glucose is +3.7 kcal/mole, calculate the standard free energy change for the combined reaction of ATP + glucose + glucose g ADP + maltose + inorganic phosphate.) it is non-spontaneous and endothermic (because the overall DGo is negative) it is spontaneous and exothermic (because the overall DGo is negative) 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 negative)arrow_forwardCalculate the equilibrium constant for the reaction glucose-1-phosphate + H2O → glucose + H2PO4− at pH 7.0 and 25°C (ΔG°′ = −20.9 kJ · mol−1).arrow_forward
- The formation of maltose, a disaccharide, from two glucose molecules, is not energetically favorable. However, if this reaction is coupled with the hydrolysis of ATP, the reaction occurs more favorably. Maltose + H2O = 2 Glucose , ΔG'o = -15.5 KJ/mol or -3.7 kcal/mol a. Determine if the coupled reaction will occur spontaneously at standard state through calculating the Gibbs Free Energy of Reaction. b. Calculate the equilibrium constant for each individual reaction, and for the coupled reaction (using free energy of reaction). Show that the equilibrium constant for the coupled reaction equals the equilibrium constants for the individual reactions multiplied together. c. If the reaction medium contains the following chemical species at their given concentrations (298 K and 1.0 atm, pH = 7.0), will the reaction proceed in the forward or the reverse direction? [Maltose] = [Glucose] = 10.0 mM; [ATP] = 5.0 mM; [ADP] = [Pi] = 20 mMarrow_forwardConsider the following chemical equation whose delta(G) = 9kcal/mol: AC + BD ---> AB + CD what are the reactants and what are the products is this reaction spontaneous? How do you know? Is energy released or consumed by this reaction? If an enzyme, which catalyzes this reaction is added, what will happen to delta (G) If this reaction is coupled to another reaction, whose delta(G) is -12 kcal/mol, what will be the net delta(G) value? will the overall reaction be spontaneousarrow_forwardThe oxidation of glucose to CO2 and water is a major source of energy in aerobic organisms. It is a reaction favored mainly by a large negative enthalpy change. C6H12O6(s) + 6O2(g) →6CO2(g) + 6H2O(l) ∆H° = -2816 kJ/mol ∆S ° = +181 J/mol . K (a) At 37 °C, what is the value for ∆G°? (b) In the overall reaction of aerobic metabolism of glucose, 32 moles of ATP are produced from ADP for every mole of glucose oxidized. Calculate the standard state free energy change for the overall reaction when glucose oxidation is coupled to the formation of ATP at 37 °C. (c) What is the efficiency of the process in terms of the percentage of the available free energy change captured in ATP?arrow_forward
- While fatty acids longer than 20 carbons are rarely found in foods, lignoceric acid (24:0) is found in a variety of tree nuts. Answer the following based on the conversion of a molecule of lignoceric acid to 8-hydroxybutyrate. (a) What are the 8-oxidation products and how many ATP are required during activation for one molecule of lignoceric acid? (b) Given the following, how many molecules of 8-hydroxybutyrate can be produced? CoA 2 2 CoA NADH NAD+ H+ OH ẞ-hydroxybutyrate (c) Based on the total NADH and FADH2 available after converting lignoceric acid into 8-hydroxybutyrate, what is the maximum yield of ATP that can be produced in the liver? Don't forget to include any ATP required for activation steps.arrow_forwardAssume that you have a solution of 0.1 M glucose 6-phosphate. To this solu- tion you add the enzyme phosphoglucomutase, which catalyzes the reaction: glucose-6-P = glucose-1-P AG' = +1.7 kJ/mol (a) Does this reaction proceed at all as written at 25 °C, and if so, what are the final concentrations of glucose 6-P and glucose 1-P? (b) What effect would omitting the enzyme have on the reaction. Be specific. (c) Under what cellular conditions, if any, would this reaction continuously produce glucose 1-P at a high rate?|arrow_forwardInside cells, the AG value for the hydrolysis of ATP to ADP + Pi is approximately -50 kJ/mol (-12 kcal/mol). Calculate the approximate ratio of [ATP] to [ADP][Pi ] in cells at 37°C. AG = AG + RT InKe R= 8.315 x 10³ kJ mol deg T= 298 K Table 15.1 Standard free energies of hydrolysis of some phosphorylated compounds Compound kJ mol- kcal mol- Phosphoenolpyruvate 1,3-Bisphosphoglycerate Creatine phosphate ATP (to ADP) -61.9 -14.8 -49.4 -11.8 -43.1 -10.3 -30.5 - 7.3 - 5.0 Glucose 1-phosphate Pyrophosphate Glucose 6-phosphate -20.9 -19.3 -4.6 -13.8 3.3 Glycerol 3-phosphate - 9.2 2.2 biochemistryarrow_forward
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