At high temperatures bromine molecules can dissociate into bromine atoms. For the reaction Br2(g) = 2 Br (g) Kp = 2.48 x 10~³ at 1650 °C. A 5.00 L vessel at 1650 °C is filled with Br2(g) at an initial pressure of 7.00 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Br·(g) at equilibrium?
At high temperatures bromine molecules can dissociate into bromine atoms. For the reaction Br2(g) = 2 Br (g) Kp = 2.48 x 10~³ at 1650 °C. A 5.00 L vessel at 1650 °C is filled with Br2(g) at an initial pressure of 7.00 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Br·(g) at equilibrium?
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
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 112CP: Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were...
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Question
![At high temperatures bromine molecules can dissociate into
bromine atoms. For the reaction
Br2(g) = 2 Br:(g)
atm
Kp = 2.48 x 10-3 at 1650 °C. A 5.00 L vessel at 1650 °C is filled
with Br2(g) at an initial pressure of 7.00 atm and allowed to come to
equilibrium. What will be the pressure (in atm) of Br (g) at
equilibrium?
1
4
6
C
LO](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf594692-d96b-4ff4-ac1a-31ce1d3fad0a%2F30cbc5f5-fb15-4e11-a153-044ff65e3902%2Fx3i56y_processed.png&w=3840&q=75)
Transcribed Image Text:At high temperatures bromine molecules can dissociate into
bromine atoms. For the reaction
Br2(g) = 2 Br:(g)
atm
Kp = 2.48 x 10-3 at 1650 °C. A 5.00 L vessel at 1650 °C is filled
with Br2(g) at an initial pressure of 7.00 atm and allowed to come to
equilibrium. What will be the pressure (in atm) of Br (g) at
equilibrium?
1
4
6
C
LO
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