For the reaction 2 NO2(g) = 2 NO(g) + O2(g) Kp = 1.11 x 10-5 at 200 °C. A 2.50 L vessel at 200 °C is filled with NO2(g) at an initial pressure of 2.75 atm and allowed to come to equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?
For the reaction 2 NO2(g) = 2 NO(g) + O2(g) Kp = 1.11 x 10-5 at 200 °C. A 2.50 L vessel at 200 °C is filled with NO2(g) at an initial pressure of 2.75 atm and allowed to come to equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 46E
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For the reaction
2 NO2(g) = 2 NO(g) + O2(g)
Kp = 1.11 × 10-5 at 200 °C. A 2.50 L
vessel at 200 °C is filled with
NO2(g) at an initial pressure of 2.75
atm and allowed to come to
equilibrium. What will be the
pressure (in atm) of NO(g) at
equilibrium?
atm
1
2
4
6.
C
7
8
+/-
x 10 0
Tap here or pull up for additional resources
3.
LO](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc14b7619-7f42-456d-bd15-e2d5f2d4f203%2F5d8f0ccc-bea8-4743-a4a9-366b545486e9%2Fr23uj2t_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Question 4 of 4
Submit
For the reaction
2 NO2(g) = 2 NO(g) + O2(g)
Kp = 1.11 × 10-5 at 200 °C. A 2.50 L
vessel at 200 °C is filled with
NO2(g) at an initial pressure of 2.75
atm and allowed to come to
equilibrium. What will be the
pressure (in atm) of NO(g) at
equilibrium?
atm
1
2
4
6.
C
7
8
+/-
x 10 0
Tap here or pull up for additional resources
3.
LO
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