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Help with chemistry problem. Equilibrium in gas reactions?
Can you help me with this problem? I have no idea how to do about doing it. I found the Kc from the Kc and the morality of the one reactant, but I don't know what do do next.
NH4HS (s) decomposes in this reaction
NH4HS (s) <----> H2S (g) + NH3 (g)
Kp=.10 at 200 degrees C
if 100.0g of NH4HS is added to a 2.0L container what is the partial pressure of NH3 at equilibrium?
2 Answers
- MuktiLv 78 years agoFavorite Answer
mol of NH4HS = 100.0g / 51.11g/mol = 1.96 mol
. . . . . . . . . .NH4HS (s) <----> H2S (g) + NH3 (g)
initial : . . . . . .1.96
change : . . . . .-x . . . . . . . . . .+x . . . . . .+x
equilibrium : . 1.96 - x . . . . . . . .x . . . . . x
since mol of H2S = mol of NH3 at equilibrium , partial pressure H2S = partial pressure NH3
Kp = P_H2S x P_NH3
10 = P_H2S x P_NH3
P_H2S = P_NH3 = sqrt10 = 3.16 atm
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- ErikaLv 45 years ago
in case you develop the stress, the equipment will respond by ability of going interior the direction that has fewer gas moles. thus, there are 2 gas moles on the two edge of the equation, so the equipment does no longer something. (selection D) because of the fact the reaction is exothermic (i.e. supplies off warmth), in case you cool it down, the equipment will respond by ability of attempting to make extra warmth (i.e. pass to the spectacular). (selection A)
