Chapter 12, Problem 12.53PAE

The decomposition of NH₄HS,

${\text{NH}}_{\text{4}}\text{HS}\left(\text{s}\right)\rightleftarrows \text{ NH3}\left(\text{g}\right)+{\text{ H}}_{\text{2}}\text{S}\left(\text{g}\right)$

is an endothermic process. Using Le Chatelier's principle, explain how increasing the temperature would affect the equilibrium. If more NH₄HS is added to a flask in which this equilibrium exists, how is the equilibrium affected?

What if some additional NH₃ is placed in the flask?

What will happen to the pressure of NH3 if some H₂S is removed from the flask?