# Problem: Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250°C:  NH4HS(s) ⇌ H2S(g) + NH3(g)If 55.0 g of NH4HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH 3(g) at equilibrium?

###### FREE Expert Solution

When dealing with equilibrium and Kp:

Kp → equilibrium units in terms of pressure
Kp is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only gaseous species are included in the equilibrium expression

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###### Problem Details

Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250°C:
NH4HS(s) ⇌ H2S(g) + NH3(g)
If 55.0 g of NH4HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH 3(g) at equilibrium?