#1
Help me answer this question, or at least tell me what I should do to solve it

Ammonium hydrogen sulfide decomposes according to the following reactions, for which Kp=0.11 at 523.15 K.

NH4HS(s)=H2S(g) + NH3(g)

If 58.3 g NH4HS(s) is placed in a sealed 3.1 L container, what is the partial pressure of NH3(g) at equilibrium?
#2
I'd determine the charages of everything in NH4HS(s)=H2S(g) + NH3(g) (many of which are probebly isotopes, which you'd have to go to the periodic table for), which will balance the equation, then it seems to get mathematical.

Don't go into chemistry.
What do we tell our children? Look before you leap. Stop and think. Don't judge a book by its cover. We believe that we are always better off gathering as much information as possible and spending as much time as possible in deliberation.
#3
i'll help u out in a bit...i'll repost once i figure/remember out how to do it...been doing this a couple of weeks ago in my ap chemistry class
Originally Posted by evening_crow
Quoting yourself is cool.


WARNING: I kill threads.
#4
okay...sorry, can't help u actually cuz my teacher sucks and never quite tought us how to do this stuff.
Originally Posted by evening_crow
Quoting yourself is cool.


WARNING: I kill threads.