Consider the following equilibrium reactions, which is the first step in the commercial process of nitric acid: Delta H: -905.6 kJ 4 NH3 (g) + 5 NO2 (aq) = 4 NO (g) + 6 H2O (g) QUESTION: How would increasing the concentration of water effect the equilibrium? Shifting it left or right?
Consider the following equilibrium reactions, which is the first step in the commercial process of nitric acid: Delta H: -905.6 kJ 4 NH3 (g) + 5 NO2 (aq) = 4 NO (g) + 6 H2O (g) QUESTION: How would increasing the concentration of water effect the equilibrium? Shifting it left or right?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section4.7: Where Does The Energy Come From?
Problem 4.14CE
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Consider the following equilibrium reactions, which is the first step in the commercial process of nitric acid:
Delta H: -905.6 kJ
4 NH3 (g) + 5 NO2 (aq) = 4 NO (g) + 6 H2O (g)
QUESTION: How would increasing the concentration of water effect the equilibrium?
Shifting it left or right? - Please explain so I can understand why!
Thank you!
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