Many metabolites are maintained at steady-state concentrations that are far from equilibrium. A comparison of Keg and Q, themass-action ratio, can determine whether a metabolic reaction is far from equilibrium.The equation for this equilibrium is,fructose 6-phosphate + ATP = fructose 1,6-bisphosphate + ADPCalculate Keg for this reaction at T = 25.0 °C.AG' = -14.2 kJ/molKeg =Calculate the mass-action ratio, Q, from the approximate physiological concentrations for rat heart tissue shown in the table.MetaboliteConcentration (µM)fructose 6-phosphate82.0Q =fructose 1,6-bisphosphate31.0АТР12,900ADP1,390

Answered: Image /qna-images/answer/b5c42011-519b-4c49-af0d-ffa8859c95b7.jpg

Many metabolites are maintained at steady-state concentrations that are far from equilibrium. A comparison of Kég and Q, the mass-action ratio, can determine whether a metabolic reaction is far from equilibrium. The equation for this equilibrium is, fructose 6-phosphate + ATP fructose 1,6-bisphosphate + ADP Calculate Ko for this reaction at T = 25.0 °C. AG' = -14.2 kJ/mol Calculate the mass-action ratio, Q, from the approximate physiological concentrations for rat heart tissue shown in the table. Metabolite Concentration (µM) fructose 6-phosphate 82.0 Q = fructose 1,6-bisphosphate 31.0 АТР 12,900 ADP 1,390

Many metabolites are maintained at steady-state concentrations that are far from equilibrium. A comparison of Kég and Q, the mass-action ratio, can determine whether a metabolic reaction is far from equilibrium. The equation for this equilibrium is, fructose 6-phosphate + ATP fructose 1,6-bisphosphate + ADP Calculate Ko for this reaction at T = 25.0 °C. AG' = -14.2 kJ/mol Calculate the mass-action ratio, Q, from the approximate physiological concentrations for rat heart tissue shown in the table. Metabolite Concentration (µM) fructose 6-phosphate 82.0 Q = fructose 1,6-bisphosphate 31.0 АТР 12,900 ADP 1,390

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...

See similar textbooks

Similar questions

With little explanation
A chemist fills a reaction vessel with 2.20 atm methane (CH4) gas, 4.05 atm oxygen ₂) gas, 3.27 atm carbon dioxide (CO₂) gas, and 7.25 atm hydrogen (H₂) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: CH₂(g) + O₂(g) → CO₂(g) + 2H₂(g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. kJ X Ś
Chp 19 #28 & # 30
Consider the following reaction. We say that this reaction is ____ and that the sign of ∆H is _____. C3H8 + 5 O2 → 3 CO2 + 4 H2O + 488 kcal
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
24
Consider these hypothetical chemical reactions: 1. A = B, 2. B = C, AG = 12.3 kJ/mol AG = -27.1 kJ/mol 3. C =D, AG = 8.50 kJ/mol What is the free energy, AG, for the overall reaction, A = D? Express your answer with the appropriate units. ► View Available Hint(s) AG = Submit LO μA Value Units ? Units input for part A