Chemistry Forum

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?

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