1
answer
2
watching
1,088
views
11 Nov 2019
Ammonium hydrogen sulfide decomposes according to the following reaction: NH4HS(s) â NH3(g) + H2S(g); Kp = 0.11 at 250oC. If 5.10 g of NH4HS(s) is placed in a sealed 5.0-L container, what are the partial pressures of NH3 and H2S when the reaction reaches equilibrium at 250oC? How many grams of NH4HS(s) remain at equilibrium? Whats the minimum volume of a container for this substance to completely decompose?
Ammonium hydrogen sulfide decomposes according to the following reaction: NH4HS(s) â NH3(g) + H2S(g); Kp = 0.11 at 250oC. If 5.10 g of NH4HS(s) is placed in a sealed 5.0-L container, what are the partial pressures of NH3 and H2S when the reaction reaches equilibrium at 250oC? How many grams of NH4HS(s) remain at equilibrium? Whats the minimum volume of a container for this substance to completely decompose?
Collen VonLv2
9 Feb 2019
Related textbook solutions
Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232
