NH4CO2NH2 (s) equilibrium reaction arrow 2 NH3 (g) + CO2 (g) Ammonium carbamate decomposes according to the equation above. At 40°C, an equilibrium mixture for this reaction contains 0.0640 atm CO2 and 0.370 atm NH3. What is the value of the equilibrium constant Kp for the reaction?

Kp = 8.76*10⁻³

Explanation:

We determine the carbamate decomposition in equilibrium:

NH₄CO₂NH₂ (s) ⇄ 2NH₃ (g) + CO₂ (g)

Let's build the expression for Kp

Kp = (Partial pressure NH₃) ². Partial pressure CO₂

We do not consider, the carbamate because it is solid and we only need the partial pressure from gases

Kp = (0.370atm) ². 0.0640 atm

Kp = 8.76*10⁻³

Remember Kp does not carry units