± Heterogeneous Equilibrium of Ammonium Bisulfide - Copy
Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction
NH4HS(s)⇌NH3(g)+H2S(g)
This reaction has a Kp value of 0.120 at 25 ∘C.
An empty 5.00-L flask is charged with 0.300 g of pure H2S(g), at 25 ∘C.
Part A
What is the initial pressure of H2S(g) in the flask?
Express your answer numerically in atmospheres.
Hints
P = |
4.31×10−2 |
atm |
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Addition of ammonium bisulfate
In addition to the H2S already present in the flask, solid NH4HS is added until there is excess unreacted solid remaining.
Part B
What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3 and PH2S, respectively?
Enter the partial pressure of ammonia followed by the partial pressure of hydrogen sulfide numerically in atmospheres separated by a comma.
NH4HS(s) <---------------------> NH3(g) + H2S(g)
0 0.0431
x 0.0431 + x
Kp = PH2S x PNH3
0.120 = x (0.0431 + x )
0.120 = 0.0431 x + x^2
X^2 + 0.0431 x - 0.120 = 0
x = 0.326
partaial pressures :
PNH3 = 0.326 atm
PH2S = 0.0431 + 0.326
PH2S = 0.369 atm
± Heterogeneous Equilibrium of Ammonium Bisulfide - Copy Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen...
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