Pro..)-The standard free energy of hydrolysis (AG) ofATP is -30.5 kJ/mole. The actual concentrations of ATP, ADP and Pi inhuman erythrocytes are 2.25 x 10-3, 2.5 x 104 and 1.65 x 10-³ M Finiog.nworlzrespectively. What is the free energy of hydrolysis of ATP at pH 7 and25 °C? -Hydrolysis of ATP can be written as: ATPnoi ADP + Pizzneswted noits219vno sri3 ni bailqmi 916 22slo ni borsvoo ver ew terli

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ATP is -30.5 kJ/mole. The actual concentrations of ATP, ADP and Pi in (log human erythrocytes are 2.25 x 10-3, 2.5 x 104 and 1.65 x 10-³ M respectively. What is the free energy of hydrolysis of ATP at pH 7 and 25 °C? -Hydrolysis of ATP can be written as: ATP 51 noi ADP+ Piz .nworl

ATP is -30.5 kJ/mole. The actual concentrations of ATP, ADP and Pi in (log human erythrocytes are 2.25 x 10-3, 2.5 x 104 and 1.65 x 10-³ M respectively. What is the free energy of hydrolysis of ATP at pH 7 and 25 °C? -Hydrolysis of ATP can be written as: ATP 51 noi ADP+ Piz .nworl

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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MISSED THIS? Read Section 19.6 (Pages 863 - 867) ; Watch KCV 19.6, IWE 19.4. Part A Consider the following reaction: 2Ca(s) + O2 (g) → 2CAO(s) AH = -1269.8 kJ; ASxn = -364.6 J/K Calculate the free energy change for the reaction at 29 °C. Express your answer using four significant figures. Assume that all reactants and products are in their standard states. NV ΑΣφ AG = kJ Submit Request Answer Part B Is the reaction spontaneous? spontaneous nonspontaneous
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a) 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?
Actual free-energy change is a function of the reactant and product concentrations and the temperature at which the reaction occurs. AG = Go + RT In Use the equation for the actual free-energy change to plot AG against In Q at 25 °C for the five concentrations of ATP, ADP, and P₁ shown in the table. The AG' for the reaction is -30.5 kJ/mol. Concentration (mm) 0.2 5.0 14.9 O O AG (kJ/mol) Metabolite ATP ADP P₁ Select the graph that plots the data. AG (kJ/mol) 0 -20 -40 -~ 0 200 0 -200 [C]c[D]d [A]a[B]b -400 T 2 5 0.2 10 2 T 4 3 2.2 12.1 InQ 6 4 InQ 6 8 1 4.2 14.1 10 8 5 25 10 AG (kJ/mol) AG (kJ/mol) 0 -20 -40 -10 -8 0 -20 -40 -6 -4 InQ -2 0
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The standard free energy change for the hydrolysis of ATP is -30.5 kJ ATP(aq)+H₂O(1)→ADP(aq) +Pi(aq) In a particular cell, the concentrations of ATP, ADP, and Pi are 0.0031 M, 0.0015 M, and 0.0048 M, respectively. Calculate the free energy change for the hydrolysis of ATP under these conditions. (Assume a temperature of 298 K.)