Suppose 15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium. At equilibrium, there is 0.03 mole of ammonium gas. What is the equilibrium constant, Kç, for the following reaction at 25°C? Please report 4 decimal places, without units. NH4HS(s) NH3(g) + H2S(g)
Suppose 15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium. At equilibrium, there is 0.03 mole of ammonium gas. What is the equilibrium constant, Kç, for the following reaction at 25°C? Please report 4 decimal places, without units. NH4HS(s) NH3(g) + H2S(g)
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 60QRT
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