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URGENT! Consider the following decomposition reaction of ammonium carbonate ((NH4)2CO3):
(NH4)2CO3 (s) 2 NH3 (g) + CO2 (g) + H2O (g)
In one experiment at 25.0°C, a sample of pure (NH4)2CO3 is placed in an evacuated 2.00 L vessel. At equilibrium, the total pressure is found to be 0.8944 atm.
(a) Determine the equilibrium partial pressure of each gaseous species.
(b) Determine the mass of ammonium carbonate ((NH4)2CO3) that must have reacted in order to achieve equilibrium.
(c) Determine the value of Kp assuming that the reaction temperature is 25.0°C.
I can find a but I am stuck at b
 one year ago
 one year ago
URGENT! Consider the following decomposition reaction of ammonium carbonate ((NH4)2CO3): (NH4)2CO3 (s) 2 NH3 (g) + CO2 (g) + H2O (g) In one experiment at 25.0°C, a sample of pure (NH4)2CO3 is placed in an evacuated 2.00 L vessel. At equilibrium, the total pressure is found to be 0.8944 atm. (a) Determine the equilibrium partial pressure of each gaseous species. (b) Determine the mass of ammonium carbonate ((NH4)2CO3) that must have reacted in order to achieve equilibrium. (c) Determine the value of Kp assuming that the reaction temperature is 25.0°C. I can find a but I am stuck at b
 one year ago
 one year ago

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AwstinfBest ResponseYou've already chosen the best response.1
use PV=nRT to find the moles and then convert back
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
but wait Im stuck with the ATM at equilibrium, the solid doesnt affect equilibrium at all, so how can I find it with the equilibrium of Pressure Don't I need concentration?
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
So you have pressure at EQ right?
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
Yeah, the total, and I can use basic mole ratio to find individual pressure
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
solve for x then use the pressure for lets say CO2 put that into PV=nRT then solve for n then convert over
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
So I need to find n for one product than just use stoichiometry ?
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
let me work it out for you really fast
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
Alright ill try it and post if it works
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
(.2236)(2)/(298*.08206) = .0183*96g/mol = 1.76g
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
I cant beleive I didnt think of that, and for C , Q goes to infinity no? How to I possible use my Equilibrium constant equation?
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
How do I possibly*
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
for C? all you do is [NH3]^2[CO2][H2O]=Kp x=.2236 (2*.2236)^2(.2236)*(.2236)=.001
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
Not for PNH3 not [NH3] for each
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
Oh I thought you had to use ICE and Q to find the direction of the reaction :/ Apparently you don't thanks a lot!
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
Q is to judge where you are in respect to K if you have a larger Q you know you have far too many products so you need to get more reactants so the reaction goes to the left, if you have a small Q you know you have too many reactants and you need to go to products. you as in the reaction lol.
 one year ago

MarcLeclairBest ResponseYou've already chosen the best response.1
Ah I get it its just to judge the direction of the reaction BEFORE equilibrium but here we already reached it! Thanks a lot!
 one year ago

AwstinfBest ResponseYou've already chosen the best response.1
Yep you got it! good luck!
 one year ago
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