The partial pressures of an equilibrium mixture of N₂O4 (9) and NO₂(g) are PN,o, = 0.33 atm and PNO, = 1.21 atm at a certain temperature. The volume of the container is doubled. Find the partial pressures of the two gases when a new equilibrium is established. Partial pressure of NO₂ = atm Partial pressure of N₂O4 M atm
The partial pressures of an equilibrium mixture of N₂O4 (9) and NO₂(g) are PN,o, = 0.33 atm and PNO, = 1.21 atm at a certain temperature. The volume of the container is doubled. Find the partial pressures of the two gases when a new equilibrium is established. Partial pressure of NO₂ = atm Partial pressure of N₂O4 M 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 73QAP
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![The partial pressures of an equilibrium mixture of N₂O4 (g) and NO₂ (g) are PN,0, = 0.33 atm and
PNO, 1.21 atm at a certain temperature. The volume of the container is doubled. Find the partial
pressures of the two gases when a new equilibrium is established.
Partial pressure of NO₂ =|
atm
Partial pressure of N₂O4
Submit Answer
Retry Entire Group
atm
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Transcribed Image Text:The partial pressures of an equilibrium mixture of N₂O4 (g) and NO₂ (g) are PN,0, = 0.33 atm and
PNO, 1.21 atm at a certain temperature. The volume of the container is doubled. Find the partial
pressures of the two gases when a new equilibrium is established.
Partial pressure of NO₂ =|
atm
Partial pressure of N₂O4
Submit Answer
Retry Entire Group
atm
8 more group attempts remaining
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