The decomposition of NH 4 HS is an endothermic process. Using Le Chateliers principle, explain how increasing
Question:
The decomposition of NH4HS
is an endothermic process. Using Le Chatelier’s principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?
Transcribed Image Text:
NH4HS(s) NH3(g) + H₂S(g)
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Increasing the temperature would shift the equilibrium to the right producing more NH3 and H2S This ...View the full answer
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Related Book For
Chemistry And Chemical Reactivity
ISBN: 9780357001172
10th Edition
Authors: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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