Step 1:

The volume of the flask is 5.0 L.

Equilibrium constant

Temperature of the hydrogen sulfide is 25 C.

Temperature in Kelvin = 25 + 273 = 298 K.

Amount of hydrogen sulfide is 0.300 g.

Convert grams into moles.

Molecular mass of the hydrogen sulfide is 34.0809 g/mol.

Number of moles of hydrogen sulfide is .

(a)

Find the initial pressure of hydrogen sulfide.

Ideal law of gas: .

Initial pressure of hydrogen sulfide 0.0392 atm.

Step 2:

Step 3:

(c)

The chemical equation is .

Equilibrium constant is

, where , and are the partial pressures.

Let x be the change in pressure.

Partial Pressure = Initial Pressure + Change in Pressure

Partial Pressure of hydrogen sulfide = 0.0392 + x

Partial Pressure of Ammonia =  x

Partial pressure of Ammonium hydro sulfide is 1.   (Since it is a solid substance)

Partial pressure cannot be negative then .

Partial Pressure of hydrogen sulfide = 0.0392 + 0.327 = 0.3662 atm.

Partial Pressure of Ammonia =  0.327 atm.

Step 4:

(d)

Total Pressure of the gas is 0.3662 + 0.327 = 0.6932 atm.

Find the mole fraction of Ammonia.

Mole fraction and Partial pressure relationship:

where

is the mole fraction of the individual gas.

is the partial pressure of the individual gas.

is the total pressure of the mixture.

Number of moles of Ammonia is 0.4717 mol.

Step 5:

(e)

Pressure of ammonia = 0.327 atm.

Now we calculate the mass of ammonia here using ideal gas equation.

Ideal law of gas: .

Now convert moles into grams.

Minimum mass of the Ammonium hydro sulfide is

Minimum mass of Ammonium hydro sulfide is3.4119 grams.

Solution :