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 0.450 g of pure H2S(g), at 25 ∘C.

Part A

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Evaluate the validity of the following statements.

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True

No reaction occurs.

The pressure of ammonia is zero.

Q is equal to 0.

False

Q is greater than K.

The reaction proceeds to the left.

The reaction proceeds to the right.

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Correct

Part B

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

Express your answer numerically in atmospheres.

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P =

6.46×10−2

atm

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Significant Figures Feedback: Your answer 0.0648 atm was either rounded differently or used a different number of significant figures than required for this part. If you need this result for any later calculation in this item, keep all the digits and round as the final step before submitting your answer.

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 C

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.

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PNH3, PH2S =

atm

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Part D

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

Express your answer numerically.

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χH2S =

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Part E

What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.450 g of pure H2S(g), at 25 ∘C to achieve equilibrium?

Express your answer numerically in grams.

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mass>

g

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