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Dinitrogen tetroxide decomposes according to N2O4(g)=2NO2(g). In a certain experiment, N2O4(g) at an initial pressure of 0.554 bar is introduced into an empty reaction container; after equilibrium is established, the total pressure is 0.770 bar. A quantity of NO2(g) is injected into the container and the total pressure jumps to 0.906 bar. Calculate the total pressure after equilibrium is reestablished.

Respuesta :

bharathparasad577

The total pressure after equilibrium will be 0.854 atm calculated  help of kp.Since the Kp depends on the individual partial pressures of the components in mixture.

N₂O₄ ==> 2NO₂

initial..0.554.........0

change....-p..........+2p

equil....0.554-p.......2p

Total Pressure at equilibrium  = 0.770;

therefore,

0.554-p+2p = 0.770 and this allows  to calculate Kp.

NO₂ is injected to make  the Ptotal equals to 0.906 bar

so that makes 0.906-0.770 = 0.136 bar  being injected.

It would make a new ICE chart with the NO₂ start = 0.136 + old equilibrium pressure of  N₂O₄ = old equilibrium and recalculate the new pressures using the Kp from the first part. You know of course that the reaction will be shifted to  left side

To know more about equilibrium  pressure, please refer;

https://brainly.com/question/25651917

#SPJ4

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