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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
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
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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 8 more group attempts remaining
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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