How Is Total Pressure Calculated in an Evacuated Rigid Container at Equilibrium?

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Total pressure in an evacuated rigid container at equilibrium can be calculated using the equilibrium constant Kp for the reaction NH4OCONH2(s) <--> 2 NH3(g) + CO2(g) at 258°C, where Kp = 2.9 x 10^-3 atm³. The concentration of the solid NH4OCONH2 does not affect the equilibrium expression, as its activity is considered to be 1. The relationship between the partial pressures of ammonia and carbon dioxide must be established to solve for total pressure. The user attempted various mathematical manipulations of Kp but found them incorrect, indicating a need for clarification on the relationship between the gases involved. Understanding how to express the total pressure in terms of the partial pressures of NH3 and CO2 is crucial for solving the problem.
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Homework Statement


At 258°C, Kp = 2.9 x 10^-3 atm3 for the following reaction.

NH4OCONH2(s) <--> 2 NH3(g) + CO2(g)

In an experiment carried out at 258°C, 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.


Homework Equations


I think its [NH4OCONH2]/[NH3]^2[CO2]=2.9 x 10^-3


The Attempt at a Solution


I tried squaring it and also taking the square root of it but neither of it was right. I also tried the reciprocal.
 
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How are pressures of ammonia and carbon dioxide related to each other?

What is the activity of solid NH4OCONH2?
 

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