Ammonium hydrogen sulfide (NH4SH) was detected in the atmosphere of Jupiter subsequent to its collision with the comet Shoemaker-Levy. The decomposition of NH4SH(s) and its equilibrium with ammonia and hydrogen sulfide is described by the following reaction:
NH4SH(s) <-> NH3(g) + H2S(g); Kp = 0.11 at 25°C. If we have a 1.00-L flask which already contains gaseous NH3 at a pressure of 0.25 atm and heat up some NH4SH, what will the equilibrium pressure of NH3 be at 25°C?
OK SO I WAS TRYING TO DO IT BUT I DON'T KNOW HOW TO APPROACH IT, IF ANYBODY KNOWS PLEASE AND THANK YOU!