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The following reaction describes the decomposition of ammonium hydrogen sulfide: NH3 (g) NH4HS (s) H2S (g) (exothermic) If a 6.1589 g sample of the solid is placed in an evacuated 4.000 L vessel at exactly 24°C. After equilibriun has been reached, the total pressure inside is 0.709 atm. Note: some solid remains in the vessel. a) What is the equilibrium constant for this reaction? b) What percentage of the solid has decomposed? c) If the volume of the vessel were doubled (constant temperature) would the remaining solid decompose, or what amount would remain?

The following reaction describes the decomposition of ammonium hydrogen sulfide: NH3 (g) NH4HS (s) H2S (g) (exothermic) If a 6.1589 g sample of the solid is placed in an evacuated 4.000 L vessel at exactly 24°C. After equilibriun has been reached, the total pressure inside is 0.709 atm. Note: some solid remains in the vessel. a) What is the equilibrium constant for this reaction? b) What percentage of the solid has decomposed? c) If the volume of the vessel were doubled (constant temperature) would the remaining solid decompose, or what amount would remain?

Chemical Principles in the Laboratory
Chemical Principles in the Laboratory
11th Edition
ISBN:9781305264434
Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Chapter42: Rate Studies On The Decomposition Of Aspirin
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The following reaction describes the decomposition of ammonium hydrogen sulfide: NH3 (g) NH4HS (s) H2S (g) (exothermic) If a 6.1589 g sample of the solid is placed in an evacuated 4.000 L vessel at exactly 24°C. After equilibriun has been reached, the total pressure inside is 0.709 atm. Note: some solid remains in the vessel. a) What is the equilibrium constant for this reaction? b) What percentage of the solid has decomposed? c) If the volume of the vessel were doubled (constant temperature) would the remaining solid decompose, or what amount would remain?
Transcribed Image Text:The following reaction describes the decomposition of ammonium hydrogen sulfide: NH3 (g) NH4HS (s) H2S (g) (exothermic) If a 6.1589 g sample of the solid is placed in an evacuated 4.000 L vessel at exactly 24°C. After equilibriun has been reached, the total pressure inside is 0.709 atm. Note: some solid remains in the vessel. a) What is the equilibrium constant for this reaction? b) What percentage of the solid has decomposed? c) If the volume of the vessel were doubled (constant temperature) would the remaining solid decompose, or what amount would remain?
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