Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250∘C:
NH4HS(s)⇌H2S(g)+NH3(g)
If 55.0 g of NH4HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium?
Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250∘C:
NH4HS(s)⇌H2S(g)+NH3(g)
If 55.0 g of NH4HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium?