Consider the following reaction: ? NH4HS(s) NH3(g) + H₂S(g) If a flask maintained at 304 K contains 0.104 moles of NH4HS(s) in equilibrium with 0.141 M NH3(g) and 6.54×10-² M H₂S(g), what is the value of the equilbrium constant at 304 K? K=

Consider the following reaction: ? NH4HS(s) NH3(g) + H₂S(g) If a flask maintained at 304 K contains 0.104 moles of NH4HS(s) in equilibrium with 0.141 M NH3(g) and 6.54×10-² M H₂S(g), what is the value of the equilbrium constant at 304 K? K=

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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Question

Consider the following reaction:
NH4HS(S) NH3(g) + H₂S(g)
If a flask maintained at 304 K contains 0.104 moles of NH4HS(s) in equilibrium with
0.141 M NH3(g) and 6.54×10-² M H₂S(g), what is the value of the equilbrium constant
at 304 K?
K =
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