Go Back   Chemistry Help Forum > Chemistry Forums > Undergraduate Chemistry Forum

Undergraduate Chemistry Forum Ask your undergraduate chemistry questions here.

Reply
 
Thread Tools Display Modes
Old Sep 14th 2017, 06:16 PM   #1
pineapplepizza
Junior Member
 
Join Date: Sep 2017
Location: California
Posts: 1
pineapplepizza is on a distinguished road
Determining partial pressure

Ammonium hydrogen sulfide, a solid, decomposes to give
NH3(g) and H2S(g). At 25C, some NH4HS(s) is placed
in an evacuated container. A portion of it decomposes,
and the total pressure at equilibrium is 0.659 atm. Extra
NH3(g) is then injected into the container, and when equilibrium
is reestablished, the partial pressure of NH3(g) is
0.750 atm.
(a) Compute the equilibrium constant for the decomposition
of ammonium hydrogen sulfide.
(b) Determine the final partial pressure of H2S(g) in the
container.

For (a), I assumed that the partial pressures of NH3 and H2S are equivalent since they have the same stoichiometry coefficient and divided the total pressure at equilibrium of 0.659 atm by 2 to find the partial pressures.
I am not sure how to approach (b). Do I assume the partial pressures of NH3 and H2S are equivalent again?
pineapplepizza is offline   Reply With Quote
Reply

  Chemistry Help Forum > Chemistry Forums > Undergraduate Chemistry Forum

Tags
equilibrium constant, partial pressure



Thread Tools
Display Modes



Facebook Twitter Google+ RSS Feed