Answer:
0.242 atm
Explanation:
The reaction is missing. I think this is the original question.
NH₄CO₂NH₂(s) ⇄ 2 NH₃(g) + CO₂(g)
This reaction has reached equilibrium at 40.0°C, and the total pressure is measured to be 0.363 atm. What is the equilibrium partial pressure of NH₃?
Let's consider the following reaction.
NH₄CO₂NH₂(s) ⇄ 2 NH₃(g) + CO₂(g)
We can find the partial pressures at equilibrium using an ICE Chart.
NH₄CO₂NH₂(s) ⇄ 2 NH₃(g) + CO₂(g)
I 0 0
C +2x +x
E 2x x
The total pressure is the sum of the partial pressures.
P = pNH₃ + pCO₂
0.363 atm = 2x + x = 3x
x = 0.121 atm
The partial pressure of NH₃ is 2x = 2 . (0.121 atm) = 0.242 atm
