The equilibrium reaction for the aqueous dissociation of acetic acid is shown below. CH3COOH(aq) = CH3COO (aq) + H+ (aq) Given the data in the table below and your knowledge of the "chemical standard state" (X) and the "biochemical standard state" (Xº'), answer parts a) to e). Gibbs free energy of formation, in units of kJ mol-¹, at T = 298.15 K AfGe AfGor CH3COOH(aq) -396.5 -369.3 0 CH3COO- (aq) H+ (aq) For the dissociation of acetic acid at 298.15 K, calculate A,Gº'. 0

The equilibrium reaction for the aqueous dissociation of acetic acid is shown below. CH3COOH(aq) = CH3COO (aq) + H+ (aq) Given the data in the table below and your knowledge of the "chemical standard state" (X) and the "biochemical standard state" (Xº'), answer parts a) to e). Gibbs free energy of formation, in units of kJ mol-¹, at T = 298.15 K AfGe AfGor CH3COOH(aq) -396.5 -369.3 0 CH3COO- (aq) H+ (aq) For the dissociation of acetic acid at 298.15 K, calculate A,Gº'. 0

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 91QRT: Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium...

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