For the aqueous reactionCH2OHキャーキャH-C-OHCH2-dihydroxyacetone phosphate glyceraldehyde-3-phosphatethe standard change in Gibbs free energy is AG°' = 7.53 kJ/mol. Calculate AG for this reaction at 298 K when[dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00600 M.AG=kJ/mol

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Answered: For the aqueous reaction CH2OH キャーキャ…

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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In biological cells, the energy released by the oxidation of foods is stored in adenosine triphosphate (ATP or ATP4). The essence of ATP's action is its ability to lose its terminal phosphate group by hydrolysis and to form adenosine diphosphate (ADP or ADP³-) ATP+ (aq) + H₂0 (1)→ ADP³- (aq) + HPO¯(aq) + H₂O+ (aq) At physiological conditions, pH = 7 and T = 310K (blood temperature), the enthalpy and Gibbs energy of hydrolysis are A, H = -20 and AG = -31, respectively. The hydrolysis of 1.00 mol of ATP, at these conditions, results in the extraction of 31 kJ of energy that can be used to do non-expansion work such as the synthesis of proteins or activation of neurons. mol Calculate the entropy of hydrolysis at pH = 7 and T = 310K
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For the aqueous reaction CH2OH H C-OH of ČH2-O P-O ČH2- dihydroxyacetone phosphate glyceraldehyde-3-phosphate the standard change in Gibbs free energy is AG" 7.53 kJ/mol. Calculate AG for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00300 M. AG = %3D kJ/mol

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