b A flask containing only NO2 at an initial pressure of 5.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. (Enter your answer to two significant figures.) Partial pressure of NO₂ = atm Partial pressure of N₂O4 = Submit atm

b A flask containing only NO2 at an initial pressure of 5.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. (Enter your answer to two significant figures.) Partial pressure of NO₂ = atm Partial pressure of N₂O4 = Submit atm

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 34QAP: At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105....

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Help me w this problem im a student

b A flask containing only NO₂ at an initial pressure of 5.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.
(Enter your answer to two significant figures.)
Partial pressure of NO2
atm
Partial pressure of N₂O4 =
Submit
=
atm

At a particular temperature, Kp = 0.85 for the reaction
N₂O4 (g) — 2NO2 (9)

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