5. One reaction that occurs in human metabolism is HO₂CCH₂CH₂CHCO₂H(aq) + NH3(aq)= | NH₂ Glutamic acid H₂NCCH₂CH₂CHCO₂H(aq) + H₂O(1) | NH₂ Glutamine For this reaction 4G° = 14 kJ at 25°C. a. Calculate K for this reaction at 25°C. b. In a living cell this reaction is coupled with the hydrolysis of ATP. (ATP(aq) + H₂O(l) → ADP(aq) + H₂PO4 (aq) AG°= -30.5 kJ/mol) Calculate 4G and K at 25°C for the following reaction Glutamic acid(aq) + ATP(aq) + NH3(aq) Glutamine(aq) + ADP(aq) + H₂PO4 (aq) [the hydrolysis of ATP] Cells use the hydrolysis of ATP, as a source of energy. Symbolically, this reaction can be written as ATP(aq) + H₂O(ADP(aq) + H₂PO4 (aq) *ATP: adenosine triphosphate. *ADP: adenosine diphosphate. AG-30.5 kJ

5. One reaction that occurs in human metabolism is HO₂CCH₂CH₂CHCO₂H(aq) + NH3(aq)= | NH₂ Glutamic acid H₂NCCH₂CH₂CHCO₂H(aq) + H₂O(1) | NH₂ Glutamine For this reaction 4G° = 14 kJ at 25°C. a. Calculate K for this reaction at 25°C. b. In a living cell this reaction is coupled with the hydrolysis of ATP. (ATP(aq) + H₂O(l) → ADP(aq) + H₂PO4 (aq) AG°= -30.5 kJ/mol) Calculate 4G and K at 25°C for the following reaction Glutamic acid(aq) + ATP(aq) + NH3(aq) Glutamine(aq) + ADP(aq) + H₂PO4 (aq) [the hydrolysis of ATP] Cells use the hydrolysis of ATP, as a source of energy. Symbolically, this reaction can be written as ATP(aq) + H₂O(ADP(aq) + H₂PO4 (aq) ATP: adenosine triphosphate. ADP: adenosine diphosphate. AG-30.5 kJ

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 56QRT

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Similar questions

In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Consider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?

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