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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

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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