Question

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 0.350 g of pure H2S(g), at 25 ∘C.

Part A: What is the initial pressure of

H2S(g) in the flask?

Part B: In addition to the

H2S already present in the flask, solid NH4HS is added until there is excess unreacted solid remaining. What are the partial pressures of

NH3 and H2S at equilibrium, that is, what are the values of PNH3and PH2S, respectively?

Part C:What is the mole fraction,

χ, of H2S in the gas mixture at equilibrium?

Part D:What is the minimum mass of

NH4HS that must be added to the 5.00-L flask when charged with the 0.350 g of pure H2S(g), at 25 ∘C to achieve equilibrium?

Answer 1