Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction: NH3(aq) + H2O <-> NH4+ + OH- ∆G0NH3(ag) = -26.6 kJ/mol ∆G0H2O = -237.1 kJ/mol ∆G0NH4+ = -79.3 kJ/mol ∆G0OH- = -157.2 kJ/mol For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?
Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction: NH3(aq) + H2O <-> NH4+ + OH- ∆G0NH3(ag) = -26.6 kJ/mol ∆G0H2O = -237.1 kJ/mol ∆G0NH4+ = -79.3 kJ/mol ∆G0OH- = -157.2 kJ/mol For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?
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 83QRT: Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate,...
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Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction:
NH3(aq) + H2O <-> NH4+ + OH-
∆G0NH3(ag) = -26.6 kJ/mol
∆G0H2O = -237.1 kJ/mol
∆G0NH4+ = -79.3 kJ/mol
∆G0OH- = -157.2 kJ/mol
For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?
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