Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br. and NOBR at 0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at equilibrium.. 2 NO(g) + Br:(g) =2 NOBr(g) NEXT (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to plve for the partial pressure. Do not combine or simplify terms.. 109 %3D O RESET (109) (0.0159) (0.0768) 2(0.0159) 2(0.0768) (0.0159) (0.0768) (x) (2x) (x) (2x)
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br. and NOBR at 0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at equilibrium.. 2 NO(g) + Br:(g) =2 NOBr(g) NEXT (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to plve for the partial pressure. Do not combine or simplify terms.. 109 %3D O RESET (109) (0.0159) (0.0768) 2(0.0159) 2(0.0768) (0.0159) (0.0768) (x) (2x) (x) (2x)
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 56QAP: Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g)...
Related questions
Question
![Consider the equilibrium system described by the chemical reaction below. For this
reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br. and NOBR at
0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at
equilibrium..
2 NO(g) + Br:(g) = 2 NOBr(g)
2
NEXT
If (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to
solve for the partial pressure. Do not combine or simplify terms..
Kp
109
%3D
RESET
(109)
(0.0159)
(0.0768)
20.0159)
2(0.0768)
(0.0159)*
(0.0768)
(x)
(2x)
(2x)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd862c25f-a636-4347-831e-84b629db5903%2Fb304805f-27e3-4d72-b704-b5c06612f48c%2Fimb3ew_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the equilibrium system described by the chemical reaction below. For this
reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br. and NOBR at
0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at
equilibrium..
2 NO(g) + Br:(g) = 2 NOBr(g)
2
NEXT
If (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to
solve for the partial pressure. Do not combine or simplify terms..
Kp
109
%3D
RESET
(109)
(0.0159)
(0.0768)
20.0159)
2(0.0768)
(0.0159)*
(0.0768)
(x)
(2x)
(2x)
![Consider the equilibrium system described by the chemical reaction below. For this
reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Brz and NOBR at
0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at
equilibrium..
%3D
2 NO(g) + Br:(g) =2 NOBr(g)
PREV
Based on your expression for Kp, solve for the equilibrium partial pressure of NO.
PNO
atm
%3D
RESET
0.0443
6.36
526
1.70 x 10-
0.0583](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd862c25f-a636-4347-831e-84b629db5903%2Fb304805f-27e3-4d72-b704-b5c06612f48c%2Fbawvb9j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the equilibrium system described by the chemical reaction below. For this
reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Brz and NOBR at
0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at
equilibrium..
%3D
2 NO(g) + Br:(g) =2 NOBr(g)
PREV
Based on your expression for Kp, solve for the equilibrium partial pressure of NO.
PNO
atm
%3D
RESET
0.0443
6.36
526
1.70 x 10-
0.0583
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry: The Molecular Science](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
![Chemistry: An Atoms First Approach](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
![Chemistry by OpenStax (2015-05-04)](https://www.bartleby.com/isbn_cover_images/9781938168390/9781938168390_smallCoverImage.gif)
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning