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

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SUMMARY

The total pressure in an evacuated rigid container at equilibrium for the reaction NH4OCONH2(s) <--> 2 NH3(g) + CO2(g) at 258°C is calculated using the equilibrium constant Kp = 2.9 x 10^-3 atm³. The relationship between the partial pressures of ammonia (NH3) and carbon dioxide (CO2) is crucial, as the equilibrium expression is given by Kp = [NH3]^2[CO2]/[NH4OCONH2]. The activity of the solid NH4OCONH2 is considered to be 1, simplifying the calculation of total pressure.

PREREQUISITES
  • Understanding of chemical equilibrium concepts
  • Familiarity with the equilibrium constant (Kp) and its application
  • Knowledge of partial pressure calculations
  • Basic principles of gas behavior in rigid containers
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  • Study the derivation and application of the equilibrium constant Kp in gas-phase reactions
  • Learn about calculating partial pressures from equilibrium concentrations
  • Explore the concept of activity in chemical reactions, particularly for solids
  • Investigate the effects of temperature on equilibrium constants
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Chemistry students, educators, and professionals involved in chemical equilibrium studies, particularly those focusing on gas-phase reactions and pressure calculations.

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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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