21. Based upon the following reactions, what would be the AG" for the formation of ATP from phosphoenolpyruvate and ADP? ATP → ADP + Pi phosphoenolpyruvate pyruvate + Pi AG" = -31.5 kJ/mol AG"=-62.2 kJ/mol

21. Based upon the following reactions, what would be the AG" for the formation of ATP from phosphoenolpyruvate and ADP? ATP → ADP + Pi phosphoenolpyruvate pyruvate + Pi AG" = -31.5 kJ/mol AG"=-62.2 kJ/mol

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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Describe how a) Mean Arterial Pressure, b) Maximal Oxygen Consumption, and c) Blood Flow are determined using its formula. In addition, you should explain what those factors are including cardiac output, stroke volume, heart rate, resistance, a-vO2 difference, etc. Describe how many ATPs can be generated by complete cycles of beta oxidation of free fatty acid with 20 carbons. You should indicate how many cycles of beta oxidation and Krebs cycle, and total number of products as well
Under standard conditions, is the oxidation of free FADH2 by ubiquinone sufficiently exergonic to drive the synthesis of ATP? (F = 96.5 kJ/V • mol) ubiquinone + 2H++ 2e¯ → ubiquinol E' = 0.045 V FAD + 2H++ 2e → FADH2 = E' -0.219 V ○ no, as oxidation of FADH2 by ubiquinone generates 33.6 kJ/mol ○ no, as oxidation of FADH2 by ubiquinone generates 50.9 kJ/mol ○ no, as oxidation of FADH2 by ubiquinone generates -25.5 kJ/mol ○ yes, as oxidation of FADH2 by ubiquinone generates -33.6 kJ/mol ○ yes, as oxidation of FADH2 by ubiquinone generates -50.9 kJ/mol
Using the data in this table, what is the AG° (in KJ/mol) for the reduction of FAD by water?
Within biological systems, there are always reactions that seem to occur when thermodynamically, they should not. An example is in the process of glycolysis (the conversion of glucose to pyruvate) which has ΔG°' = 2183.6 kJ/mol. How is glycolysis possible with such a large, positive ΔG°', when cells are governed by the laws of thermodynamics?
8
During glycolysis, glucose is converted into fructose-6- phosphate in two successive reactions: glucose + ATP glucose 6-phosphate + ADP glucose 6-phosphate fructose 6-phosphate The AG' for the overall reaction is: +15.0 kJ/mol. -18.4 kJ/mol. -16.7 kJ/mol. → -15.0 kJ/mol. +18.4 kJ/mol. AG¹⁰ = -16.7 kJ/mol AG¹⁰ = +1.7 kJ/mol
Calculate the standard free-energy change, deltaG'o, for the reaction in which acetaldehyde is reduced by the biological electron carrier NADH in the reaction acetaldehyde + NADH + H+ → ethanol + NAD+. Then calculate the actual free-energy change, deltaG, when the acetaldehyde is 1.51 M, the NADH is 1.02 M, the ethanol is 0.13 M and the NAD+ is 0.19 M, at 33.35oC and pH = 7. Give the actual free-energy change in kJ/mol to one decimal place. See Table 13-7b for the E'o values. please provide comprehensive explaination with each step.
The free energy change of each step of glycolysis is given in the table below. ∆G°’ is the free energy under standard conditions (25°C, 1M each reactant, pH 7), while ∆G is the free energy change at presumed physiological conditions. Why must no step have a positive ∆G under physiological conditions?
ATP Hydrolysis: ATP to ADP+Pi Given that the standard free energy change of ATP hydrolysis is –30.5 kJ/mol, what is the change in free energy in a cell at 37 °C where the ATP and Pi are both 10 mM and ADP is 10 uM?
The table contains the standard free energies of hydrolysis of phosphorylated compounds. Use the values in the table to answer questions about phosphorylation reactions in glycolysis. Compound kJ mol-1 kcal mol-1 Phosphoenolpyruvate -61.9 -14.8 1,3-Bisphosphoglycerate -49.4 -11.8 Creatine phosphate -43.1 -10.3 ATP (to ADP) -30.5 -7.3 Glucose 1-phosphate -20.9 -5.0 Pyrophosphate -19.3 -4.6 Glucose 6-phosphate -13.8 -3.3 Glycerol 3-phosphate -9.2 -2.2
Calculate the standard free-energy change, deltaG'o, for the reaction in which acetaldehyde is reduced by the biological electron carrier NADH in the reaction acetaldehyde + NADH + H+ → ethanol + NAD+. Then calculate the actual free-energy change, deltaG, when the acetaldehyde is 1.51 M, the NADH is 1.02 M, the ethanol is 0.13 M and the NAD+ is 0.19 M, at 33.35oC and pH = 7. Give the actual free-energy change in kJ/mol to one decimal place. See Table 13-7b for the E'o values.
In glycolysis, fructose 1,6-bisphosphate is converted to two products with a standard free- energy change (AG) of 23.8 kJ/mol. Under what cellular conditions will the free-energy change be negative, enabling the reaction to proceed spontaneously to form products? O In a cell where the concentrations of products and reactants yield a low value of the mass-action ratio Q ○ The reaction will not go to the right spontaneously under any conditions because the AG is positive ○ The reaction will proceed spontaneously to the right if there is a high concentration of products relative to the concentration of fructose 1,6-bisphosphate ○ The reaction will proceed spontaneously to the right if there is a high concentration of enzyme to catalyze the reaction O None of these conditions is sufficient