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(a)
Interpretation:
The stability of
Concept introduction:
Gibbs free energy is the useful work obtained from the system. It is the difference between the enthalpy and the product of entropy and absolute temperature. It is always negative. Therefore, more negative the gibbs free energy more stable the compound.
(b)
Interpretation:
The hydration reaction between
Concept introduction:
In hydration reaction, water molecules attack on a compound and it is an exothermic reaction. The molecule has standard activation energy to get hydrated. Lower the activation energy faster will be the hydration of that molecule.
(c)
Interpretation:
The free-energy-diagrams representing the hydration reaction of
Concept introduction:
Gibbs free energy is the useful work obtained from the system. The free energy diagram represents the gibbs free energy of reactants and products. The lower the gibbs free energy more stable the compound.
(d)
Interpretation:
The difference in the standard free energies of the transition states for the hydration reactions of
Concept introduction:
Gibbs free energy is the useful work obtained from the system. In hydration, the compound reacts with water to release energy. Hydration reaction has activation energy. Higher the activation energy, lower will be the
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Chapter 4 Solutions
Organic Chemistry Study Guide and Solutions
- Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.arrow_forwardFor the reaction CO(NH2)2 +H2O(l) -> CO2(g) + 2NH3(g) The ∆S^2 and ∆H^2 is 354.8KJ/mol and 119.2KJ/mol respectively. Calculate (a) the standard entropy of urea(b) the standard enthalpy of formation of urea(c) the standard free energy change of the reaction and (d) the standard free energy of formation of urea.arrow_forwarda) 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?arrow_forward
- 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.arrow_forwardWhich statement is FALSE? (A) If a reaction is thermodynamically spontaneous it may occur slowly. (B) Activation energy is a kinetic quantity rather than a thermodynamic quantity. (C) If a reaction is thermodynamically spontaneous it may occur rapidly. (D) If a reaction is thermodynamically spontaneous, it must have a low activation energy. (E) If a reaction is thermodynamically nonspontaneous, it will not occur spontaneously.arrow_forwardPlease answer this question. For the aqueous reaction: dihydroxyacetone phosphate ↽−−⇀ glyceraldehyde−3−phosphatedihydroxyacetone phosphate the standard change in Gibbs free energy is Δ?°′=7.53 kJ/molΔG°′=7.53 kJ/mol. Calculate ΔG for this reaction at 298K when [dihydroxyacetone phosphate]=0.100 M and [glyceraldehyde-3-phosphate]=0.00200arrow_forward
- A student determines the value of the equilibrium constant to be 3.67×10-18 for the following reaction. Fe3O4(s) + 4H₂(g) →→→3Fe(s) + 4H₂O(g) Based on this value of Keq: AGO for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 1.67 moles of Fe3O4(s) at standard conditions at 298K. AGᵒrxn KJarrow_forwardA student determines the value of the equilibrium constant to be 1.98×10-5 for the following reaction.CO2(g) + H2(g)CO(g) + H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 1.74 moles of CO2(g) at standard conditions at 298K. G°rxn = kJarrow_forwardin a particular solution at 30 degrees celcius the ratio of beta-d-glucose to linear glucose is 320:1. Calculate gibbs free energy at standard state for conversion of linear to beta-d-glucose. (R=8.3145 J mol-1 K-1)arrow_forward
- [2] [a] The forward reaction is spontaneous for a particular reversible reaction. What can you conclude about the reverse reaction? AG = [b] What does the sign of the free energy have to be such that a reaction is spontaneous? AS = [c] [i] Under what conditions of enthalpy and entropy change is a reaction always spontaneous? AH= [ii] Under what conditions of enthalpy and entropy change is a reaction never spontaneous? - ΔΗ AS [d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high temperature or a low temperature? [e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low temperature be more likely to lead to a spontaneous reaction?arrow_forwardThe standard free energy change for the reaction CH4(g)+2O2(g) -> CO2(g) + 2H2O(l) is -194.8 kcal at 25ºC and -191.82 kcal at 75ºC. Calculate the heat of reaction at 25ºC.Ans: -212.6 kcalarrow_forwardIn 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?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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