The essence of ATP's action in biological processes is its ability to lose its terminal phosphate group by hydrolysis forming adenosine diphosphate, ADP3-, i.e., ATP4 a (aq) + H2O (ad →ADP3 + HPO4 + H3O+( (ag) If the value of A,G° for this reaction at 300 K and pH 7 is -30.5 kJ/mol, determine AG when [ATP4] = (4.10x10^-5) M, [ADP3-] = (3.1000x10^-4) M, [HPO42]= (2.500x10^-2) M at pH 7.15. (Enter the value for AG in units of kJ/mol to 3 sig figs in the space provided.) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10

The essence of ATP's action in biological processes is its ability to lose its terminal phosphate group by hydrolysis forming adenosine diphosphate, ADP3-, i.e., ATP4 a (aq) + H2O (ad →ADP3 + HPO4 + H3O+( (ag) If the value of A,G° for this reaction at 300 K and pH 7 is -30.5 kJ/mol, determine AG when [ATP4] = (4.10x10^-5) M, [ADP3-] = (3.1000x10^-4) M, [HPO42]= (2.500x10^-2) M at pH 7.15. (Enter the value for AG in units of kJ/mol to 3 sig figs in the space provided.) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10

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

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
a Calculate K1, at 25C for phosphoric acid: H3PO4(aq)H+(aq)+H2PO4(aq) b Which thermodynamic factor is the most significant in accounting for the fact that phosphoric acid is a weak acid? Why ?
Plants synthesize carbohydrates from CO2 and H2O by the process of photosynthesis. For example, 6CO2(g)+6H2O(l)C6H12O6(aq)+6O2(g) G=2.87103 kJ at pH 7.0 and 25°C. What is K for the reaction at 25°C?
5. One of the key steps in the tricarboxylic acid (TCA) cycle is the hydration of fumarate to malate: Fumarate-² + H₂O = Malate-2 The standard reaction Gibbs free energy and enthalpy for this reactions are -880 cal/mol and 3560 cal/mol, respectively. (a) What is the equilibrium constant for this reaction (25 °C)? (b) Is the reaction favorable (spontaneous) at 25 °C? (c) What is the equilibrium constant of this reaction under physiological conditions (37 °C)? (d) Is this reaction favorable at 37 °C?
Consider the following reaction at 100.0 °C: Al(s) + NaOH(aq) + H20(l) ⇄ Na[Al(OH)4](aq) + H2(g) A) Write a balanced equilibrium quotient (Qc) for the following reaction. B) If the pressure of this reaction is increased, which direction will the equilibrium shift? Why?
At 298 K, AG° = +20.9 kJ/mol for the reaction CH;CO,H (aq) = H"(aq) + CH;CO, Calculate AG for this reaction if the [H"]= 3.19 x 10³, [CH;CO,]= 7.67 x 10, and [ CH;CO,H] = 7.47 x 10-5.
Given the following ionic equilibria and their K values: AgBr(s) ⇌ Ag+(aq) + Br–(aq); Ksp = 5.0 x 10–13 Ag+(aq) + 2NH3(aq) ⇌ Ag(NH3)2+(aq); Kf = 1.7 x 107 What is Kc for the following equilibrium? AgBr(s) + 2NH3(aq) ⇌ Ag(NH3)2+(aq) + Br–(aq); (A) 8.5 x 10–6 (B) 2.9 x 10–20 (C) 3.4 x 1019 (D) 1.7 x 107
Calculate K for the reaction Ag₂ Q(8) + CO(g) ⇒ 2 Ag(s) + CO₂ (g) given the following information: K = Ag₂ O(s) + H₂ (g) ≥ 2 Ag(s) + H₂O(g) K₁ = 1.01 X 10¹3 H₂ (g) + CO₂ (g) ⇒ H₂ O(g) + CO(g) K2 = 0.771
Use data to compute AG° at 89.0°C for the following reaction. 3N2H4() + 403(g) → 6NO(g) + 6H2O(1) AH°¢ (N2H4(1)) = 50.6 kJ mol 1 AH°t (O3(g)) = 142.7 kJ mol 1 AH°; (NO(g)) = 91.3 kJ mol-1 AH°f (H2O(1)) = -285.83 kJ mol1 AS° (N2H4()) = 121.2 J mol-1 K-1 AS° (O3(g)) = 238.9 J mol-1 K1 AS° (NO(g)) = 210.8 J mol-1 K-1 AS° (H20(1)) = 69.95 J mol-1 K-1 AG°f (N2H4(1)) = 149.3 kJ mol 1 AG°t (O3(g)) = 163.2 kJ mol1 AG°f (NO(g)) = 87.6 kJ mol-1 AG°t (H2O(1)) = -237.1 kJ mol 1 %3D %3D %3D AG° = i kJ
5 ml of a 0.2 M NH3 solution are added to 5 ml of a 0.1 M NH4Cl solution (Kb for NH3 is = 1.8 × 10-5). Calculate: a) the pH of the resulting solution; b) the ΔpH due to the addition of 5 ml of a 0.01 M HNO3 solution to the solution resulting from part a); c) the ΔpH due to the addition of 10 ml of water to the solution resulting from part a)
Use the systematic treatment of equilibrium to calculate the concentration of Ba2+ in acidic solution, if its concentration is governed by the following equilibria – BaSO4 (s) → Ba2+ + So Ksp = 1.1 x 10-10 so, +H2O HSO, +OH K, = 9.8 x 10-13 Bat + So, BaSO4 (aq) K = 1.9 x 10 Hint: Since the pH is fixed at 1.89, the charge balance is invalidated. Use the mass balance for your calculation.
kp and delta G ^ 0 IS NEEDED only

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS