Question

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 25.0ÁC, 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 25.0ÁC.

Answer 1

Using PV=nRT to find the moles and then convert back.
4x=.8944
solve for x then use the pressure for lets say CO2 put that into PV=nRT then solve for n then convert over.

(.2236)(2)/(298*.08206) = .0183*96g/mol = 1.76g

For C:

[NH3]^2[CO2][H2O] = Kp
x=0.2236 (2*.2236)^2(.2236)*(.2236)
=0.001