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Ammonium hydrogen sulfide decomposes according to the following reaction, for which

 

 

If 49.7 g of is placed in a sealed 5.0-L container, what is the partial pressure of at equilibrium?

 

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Matt Ocampo
Matt OcampoLv10
19 Jan 2021

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Related questions

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?

Ammonium hydrogen sulfide decomposes according to the followingreaction, for which Kp = 0.42 at a given temperature. If 55.0 g ofNH4HS is sealed inside a 5.00 L container at this temperature,calculate the partial pressure of NH3(g) at equilibrium: NH4HS(s)<=> NH3(g) + H2S(g)

Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9.30x10-8 at 700 degrees Celsius.

2H2S(g) → 2H2(g) + S2(g)

If 0.29 moles of H2S is placed in a 3.0-L container, What is the equilibrium concentration of H2(g) at 700 degrees Celsius?

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