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28 Nov 2019

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 0.450g of pure H2S(g), at 25 ?C.

What is the initial pressure of H2S(g) in the flask?

Express your answer numerically in atmospheres.

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Elin Hessel
Elin HesselLv2
3 Jan 2019

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Related questions

Part A. An empty 5.00-L flask is charged with 0.250 g of pure H2S(g), at 25 °C.

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.

a) What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3 and PH2S, respectively?

b)What is the mole fraction, χ, of H2S in the gas mixture at equilibrium?

c)What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.250 g of pure H2S(g), at 25 °C to achieve equilibrium? Express your answer numerically in grams.

For the reaction NH3 (g) + H2S(g) <--> NH4HS (s)

K = 400. at 35.0°C. If 2.00 mol each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium?

mass NH4HS at equilibrium =_________ g

PH2S = ____________atm

Ammonium hydrogen sulfide decomposes according to the following reaction: NH4HS(s) ⇌ 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?

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