The hydrolysis reaction, ATP + H 2O ADP + phosphate, has a standard free energy, ΔGoʼ, of -30.5 kJ/mol. (a) or (c) Show the formula for the equilibrium constant, K eq, for this reaction and give its value. Right: Effect of Mg 2+ concentration on the free energy of hydrolysis of ATP (DG ATP) at pH 7.0. Note that for ATP synthesis, the reaction is written in the reverse direction, and the sign of the free energy change is reversed, so that: ADP + inorganic phosphate (Pi) <=> ATP + H 2 O DG o ' = +7.3 kcal. mol-1
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Terms in this set (12) The standard free energy change for the hydrolysis of ATP to ADP and inorganic phosphate (Pi) is about -30 kJ/mol but in the red blood cell the actual free energy change for this reaction is about -52 kJ/mol.
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Conversion of glutamate to glutamine ∆G = +3.4kcal/mol Hydrolysis of ATP to ADP + Pi release more free energy than is consumed by glutamine synthesis-Net free energy change indicates that coupled reaction would be spontaneous Coupled reaction mechanism in cells is different from 2 separate reactions Enzymes: -Binds both ATP and glutamic acid -Transfer terminal phosphate from ATP to glutamic ...
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The hydrolysis of ATP to yield ADP and phosphate is highly exergonic. This loss of free energy is due to the structure of the phosphoanhydride, which involves two negatively charged groups being brought into close proximity. Additionally, the phosphate group is stabilized by resonance not available to the anhydride (see Figure 1). Figure 1 Aug 05, 2009 · The standard free energy change for the hydrolysis of ATP is -30.5 kJ. In a particular cell, the concentrations of ATP, ADP, and Pi are 2.8×10^-3 M, 1.2×10^-3 M, and 4.0×10^-3 M, respectively
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Since under physiological conditions an ATP hydrolysis gives free energy ≈ 20 k B T and k (+) and k (−) are constants independent of the NL strain and external force (see above), it is a good approximation to consider the transitions of the ATPase activity to be irreversible under any external force, i.e., to ignore the reverse transitions ... A. Find the equilibrium constant K for the biologically important hydrolysis reaction: ATP --> ADP + phosphate, which has. DG°=6.9 kcal/mol. B. Calculate the free energy change for this reaction when [ADP] = 0.5 x 10-3, [phosphate] = 1.0 x 10-3, and [ATP] = 5 x 10-3. These are the concentrations that occur in a typical muscle cell. Hydrolysis of adenosine triphosphate (ATP) is the “energy source” for a variety of biochemical processes. In the present work, we address key features of ATP hydrolysis: the relatively moderate value (about −10 kcal/mol) of the standard free energy, ΔG hyd, of reaction and the insensitivity of ΔG hyd to the number of excess electrons on ...
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More free energy (higher G) Less stable Greater work capacity Less free energy (lower G) More stable Less work capacity In a spontaneously change The free energy of the system decreases (∆G<0) The system becomes more stable The released free energy can be harnessed to do work (a) (b) (c) Figure 8.5 Figure 8.6 Reactants Products Energy ... The standard free energy change for the hydrolysis of ATP to ADP and inorganic phosphate (Pi) is about -30 kJ/mol but in the red blood cell the actual free energy change for this reaction is about -52 kJ/mol.
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If the DGo for ATP hydrolysis into ADP + inorganic phosphate is -7.3 kcal/mole, and the DGo for maltose synthesis from glucose + glucose is +3.7 kcal/mole, calculate the standard free energy change for the combined reaction of ATP + glucose + glucose g ADP + maltose + inorganic phosphate. A) The free-energy change (Delta G) of the hydrolysis of ATP to ADP and Pi may vary considerably with variations in pH, temperature, atmospheric pressure, and concentrations of reactants and...
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ATP is the universal currency of free energy. ATP hydrolysis drives metabolism by shifting the equilibrium constant of coupled reactions. There is a structural basis for the high phosphoryl transfer potential of ATP. The phosphoryl transfer potential is an important form of cellular energy transformation. 7. Muscles are powered by the hydrolysis of ATP to ADP + Pi. The G´ for hydrolysis of ATP is -8500 cal mol-1. At the beginning of exercise the G for the reaction is -13,200 cal mol-1, and the ATP concentration is 10 times that of ADP. But in general, the hydrolysis of ATP produces energy in excess of the energy needed for biosynthesis reactions, such as this one. So essentially what I'm saying is that if we add a very large negative number to a smaller positive number, we will get an overall negative delta G value.
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We can calculate the actual Gibbs free energy change for ATP hydrolysis (to ADP) given the known concentrations of reactants and products in rat hepatocytes. The answer is ΔG = -48 kJ mol -1. Thus, the actual Gibbs free energy change is 1½ times the standard Gibbs free energy change.A direct measurement of the standard free-energy change associated with the hydrolysis of ATP is technically demanding because the minute amount of ATP remaining at equilibrium is difficult to measure accurately.• Although the hydrolysis of ATP is highly exergonic (ΔG°´ = -30,5 kJ/mol), the ATP is stable at pH 7, because the activation energy for ATP hydrolysis is relatively high. Rapid hydrolysis of ATP occurs only when catalyzed by an enzyme. • The free energy change for ATP hydrolysis is -30,5 kJ/mol under standard conditions but the actual free
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As with most cases of ATP hydrolysis, a phosphate from ATP is transferred onto another molecule. In a phosphorylated state, the Na + /K + pump has more free energy and is triggered to undergo a conformational change. This change allows it to release Na + to the outside of the cell. Conversely, if the [ATP] was increased, then the ∆G for ATP hydrolysis would increase, making excessive free energy release and increased heat production, as well as a limited potential to reform ATP due to the diminished possibility for coupling to reactions that were at least equally free energy releasing compared to the free energy need for forming ATP.
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Dec 11, 2016 · Energy generation is driven by whatever an organism utilizes as an energy source whereas the ATP, once produced, is used to power the organism. The figure presented shows the structures of ATP and ADP but not the water molecule involved in hydrolysis as well dehydration synthesis, nor the inorganic phosphate that is added to ADP to produce ATP.
2. The energy required for packaging neurotransmitters into vesicles is provided, indirectly, from the hydrolysis of ATP. The standard free energy change for ATP hydrolysis is 30kJ=mol. Assume that the intracellular concentrations of ATP, ADP and inorganic phosphate are 2.6, 0.7 and 2.7mM, respectively. • ATP hydrolysis results in the formation of ADP and P i, and releases a large amount of free energy in the process. • ATP hydrolysis can be coupled to endergonic reactions in a cell to power hundreds of reactions.
The Gibbs energy change under such conditions (temperature 310 o K, or 37 o C) will be = o ' + 2.3 RT log ( C ADP C P i C H + / C ATP ) = -30 - 19.6 = - 49.6 kJ mol-1 This figure, calculated from the actual concentrations of the reaction components, reflects the energy available as a driving force for any other process coupled to ATP hydrolysis under given conditions. Hydrolysis is the process of breaking complex macromolecules apart. During hydrolysis, water is split, or lysed, and the resulting hydrogen atom (H +) and a hydroxyl group (OH –), or hydroxide, are added to the larger molecule. The hydrolysis of ATP produces ADP, together with an inorganic phosphate ion (P i), and the release of free energy.
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Inorganic phosphate content and free energy change of ATP hydrolysis in regional short-term hibernating myocardium. Martin C(1), Schulz R, Rose J, Heusch G. Author information: (1)Abteilung für Pathophysiologie, Zentrum für Innere Medizin des Universitätsklinikums, Essen, Federal Republic of Germany. [email protected]