-mare-foiorite 12 23. A flask is charged with 1.500 atm of N₂O4(g) and 1.00 atm NO₂(g) at 25°C, and the following equilibrium is established. 2 NO₂(g) N₂O4(g) At equilibrium, the partial pressure of NO₂(g) is 0.512 atm. Calculate the equilibrium constant Kp for this reaction. A. 9.45 B. 5.72 C. 7.58 D. 3.81 E. 6.65 2N02= N₂0 u I 1.5 с G
-mare-foiorite 12 23. A flask is charged with 1.500 atm of N₂O4(g) and 1.00 atm NO₂(g) at 25°C, and the following equilibrium is established. 2 NO₂(g) N₂O4(g) At equilibrium, the partial pressure of NO₂(g) is 0.512 atm. Calculate the equilibrium constant Kp for this reaction. A. 9.45 B. 5.72 C. 7.58 D. 3.81 E. 6.65 2N02= N₂0 u I 1.5 с G
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 91QRT
Related questions
Question
![-more-fuiorite
12
23. A flask is charged with 1.500 atm of N₂O4(g) and 1.00 atm NO₂(g) at 25°C, and the following
equilibrium is established.
2 NO₂(g) N₂O4(g)
At equilibrium, the partial pressure of NO₂(g) is 0.512 atm. Calculate the equilibrium constant
Kp for this reaction.
A. 9.45
B. 5.72
C. 7.58
D. 3.81
E. 6.65
2N02= N₂0 u
I 1.5
с
E](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5a07e433-7e70-471c-93cb-a6727fcb457b%2Facbb8584-d157-4520-84b4-95e308995363%2Fd4adwp7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:-more-fuiorite
12
23. A flask is charged with 1.500 atm of N₂O4(g) and 1.00 atm NO₂(g) at 25°C, and the following
equilibrium is established.
2 NO₂(g) N₂O4(g)
At equilibrium, the partial pressure of NO₂(g) is 0.512 atm. Calculate the equilibrium constant
Kp for this reaction.
A. 9.45
B. 5.72
C. 7.58
D. 3.81
E. 6.65
2N02= N₂0 u
I 1.5
с
E
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