The equilibrium constant, K, for the following reaction is 1.80x10-4 at 298 K. NH4HS(s) NH3(g) + H₂S(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.366 mol NH4HS, 1.34×10- 2 M NH3 and 1.34x10-2 M H₂S. If the concentration of NH3(g) is suddenly increased to 2.41x10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H₂S] = M M
The equilibrium constant, K, for the following reaction is 1.80x10-4 at 298 K. NH4HS(s) NH3(g) + H₂S(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.366 mol NH4HS, 1.34×10- 2 M NH3 and 1.34x10-2 M H₂S. If the concentration of NH3(g) is suddenly increased to 2.41x10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H₂S] = M M
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 60QRT
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