the partial pressures are the same ratio as the product moles from the reaction equation
p CO₂ = 2/9 * 2.50 atm
p N₂ = 1/3 * 2.50 atm
p H₂O = 4/9 * 2.50 atm
I have been going at part B of this problem for a few hours. I've completed an ice table and calculated the total number of moles based off pressure but am still unable to come up with the partial pressures. If someone could provide the steps for solving I would appreciate it.
4. Consider the following reaction used as a rocket fuel:
(CH3)2N2H2 (s) + N2O4 (l) ⇌ 2CO2 (g) + 3N2 (g) + 4H2O (g)
Kp for this reaction is so large you can assume it goes to completion. The gases produced by this reaction were
collected in a closed, 118 L vessel, and at equilibrium, the total pressure was 2.50 atm and the temperature was
400 K.
a) Write the equilibrium constant expression (Kp) for this reaction.
b) What are the partial pressures of CO2, N2, and H2O at equilibrium?
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