Ammonium bisulfide forms ammonia and hydrogen sulfide through the reaction NH4HS

Question

Ammonium bisulfide forms ammonia and hydrogen sulfide through the reaction

NH4HS(s)<---->NH3(g)+H2S(g)

This reaction has a Kp value of 0.120 at 25C. An empty 5.00L flask is charged with .0250 g of pure H2S at 25 degrees C. In addition to the H2S already present in the flask, solid NH4HS is added until there is excess unreacted solid remaining.

1) What are the partial pressure of NH3 and H2S at equilibrium, that is, what are the values of PNH3 and PH2S respectively

2) What is the mole fraction, X, of H2S in the gas mixture at equilibrium?

3) What is the minimum mass of NH4HS that must be added to the 5.00L flask when charged with the 0.250g of pure H2S(g) at 25 degrees C to achieve equilibrium?

Explanation / Answer

Reaction is exothermic so:
NH4HS (s) <===> NH3 (g) + H2S (g) + q
Which means when you raise temperature heat will be produced so equilibrium goes to left which means H2S will be consumed.
When you add NH4HS, it will be consumed and H2S will be produced.
About last part when you increase volume pressure decreases so more gas should be produced to increase pressure so H2S and NH3 will be produced so correct answer would be ii and iii.
Answer to question no 43:
Well when container expands volume increases hence pressure drops.so the equation goes to the side with more gas moles.
4NH3 (g) + 5O2 (g) <===> 4NO (g) + 6 H2O (g)
The right side has 10 moles of gas,so equation goes to right side which means the forward reaction rate is more than backward.

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