For the decomposition of ammonium carbamate
NH₄(NH₂CO₂) (s) ⇌ 2 NH₃(g) + CO₂(g)
K_p = 0.0596 at a certain temperature.A solid sample of ammonium carbamate is introduced into an evacuated container and at equilibrium some solid remains in the container.What is the total pressure in the container?

Question

Quizplus · Accepted Answer

The total pressure in the container can be calculated using the equilibrium constant (Kp) for the decomposition reaction. Given that Kp = 0.0596, and the reaction produces 2 moles of NH3 and 1 mole of CO2 for every mole of ammonium carbamate that decomposes, the total pressure is determined by the partial pressures of NH3 and CO2 at equilibrium. Since the reaction produces 3 moles of gas in total and some solid remains, indicating the reaction has not gone to completion, the equilibrium condition can be represented as Kp = (P_NH3)^2 * P_CO2. Given the stoichiometry of the reaction, P_NH3 is twice that of P_CO2 at equilibrium. By solving the equilibrium expression for the total pressure (P_total = 2P_NH3 + P_CO2) and using the value of Kp, the total pressure is calculated to be approximately 0.738 atm, assuming ideal behavior of the gases involved.

For the Decomposition of Ammonium Carbamate