How can we calculate the equilibrium constant KP for the decomposition of ammonium carbamate?
We know that ammonium carbamate, NH4CO2NH2, decomposes as follows:
NH4CO2NH2 (s) ⥫⥬ 2NH3 (g) + CO2 (g)
Starting with only the solid, it is found that at 40°C the total gas pressure (NH3 and CO2) is 0.363 atm.
Can you help us calculate the equilibrium constant KP for this reaction?
Calculating the equilibrium constant KP for the decomposition of ammonium carbamate
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Re: Calculating the equilibrium constant KP for the decomposition of ammonium carbamate
We have ratio 2 part ammonia to 1 part carbon dioxide
So the pressure are the same 2p NH3 + p CO2 = 0,363 atm
Kp = (2/3p)^2 *1/3 p
So the pressure are the same 2p NH3 + p CO2 = 0,363 atm
Kp = (2/3p)^2 *1/3 p