Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250ºC: 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 NH3(g) at equilibrium

0.33 atm

Explanation:

Equation for the reaction is expressed as follows:

     ⇄    

= 0.11

The equilibrium constant for the reaction can be represented as:

=

= 1   since it is solid and solid and it is known that any solid has uniformity at equilibrium.

So; =

At equilibrium ;

Let x =

So;

=

=

atm

Therefore,  the partial pressure of NH3(g) at equilibrium = 0.33 atm

2b2t

explanation:

2b2t