Respuesta :
The question is incomplete, here is the complete question:
At 25°C, Kp = 2.9 × 10⁻³ for the reaction:
[tex]NH_4OCONH_2(s)\rightleftharpoons 2NH_3(g)+CO_2(g)[/tex]
In an experiment carried out at this temperature, a certain amount of NH₄OCONH₂ is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium.
Answer: The total pressure in the container at equilibrium is 0.2694 atm
Explanation:
Let the initial concentration of [tex]NH_4OCONH_2[/tex] be 'x'
The given chemical equation follows:
[tex]NH_4OCONH_2(s)\rightleftharpoons 2NH_3(g)+CO_2(g)[/tex]
Initial: x
At eqllm: x-y 2y y
The expression of [tex]K_p[/tex] for above equation follows:
[tex]K_p=(p_{NH_3})^2\times p_{CO_2}[/tex]
The partial pressure of pure solids and liquids are taken as 1 in equilibrium constant expression. So, the partial pressure of [tex]NH_4OCONH_2[/tex] is not seen in the expression.
We are given:
[tex]K_p=2.9\times 10^{-3}[/tex]
Putting values in above expression, we get:
[tex]2.9\times 10^{-3}=(2y)^2\times y\\\\y=0.0898[/tex]
So, the equilibrium partial pressure of ammonia = 2y = (2 × 0.0898) = 0.1796 atm
The equilibrium partial pressure of carbon dioxide = y = 0.0898 atm
Total pressure inside the container at equilibrium = [tex]p_{NH_3}+p_{CO_2}=[0.1796+0.0898]=0.2694atm[/tex]
Hence, the total pressure in the container at equilibrium is 0.2694 atm
