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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: INEEDHELP2DAy on May 06, 2009, 11:43:00 PM

Title: PRESSURE PROBLEMS
Post by: INEEDHELP2DAy on May 06, 2009, 11:43:00 PM

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!

Title: Re: PRESSURE PROBLEMS
Post by: Rabn on May 07, 2009, 03:08:12 AM

It's an equilibrium problem; I.C.E. Chart.