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At high temperatures, bromine molecules can dissociate into bromine atoms. For the reaction Br₂(g) 2 Br (g) Kp = 2.48 x 103 at 1650 °C. A 5.00 L vessel at 1650 °C is filled with Br,(g) at an initial pressure of 9.00 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 103 at 1650 °C. A 5.00 L vessel at 1650 °C is filled with Br,(g) at an initial pressure of 9.00 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Br. (g) at equilibrium?

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 3PS: Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A...
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At high temperatures, bromine molecules can dissociate into bromine atoms. For the reaction Br₂(g) 2 Br (g) Kp = 2.48 x 103 at 1650 °C. A 5.00 L vessel at 1650 °C is filled with Br₂(g) at an initial pressure of 9.00 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Br. (g) at equilibrium?
Transcribed Image Text:At high temperatures, bromine molecules can dissociate into bromine atoms. For the reaction Br₂(g) 2 Br (g) Kp = 2.48 x 103 at 1650 °C. A 5.00 L vessel at 1650 °C is filled with Br₂(g) at an initial pressure of 9.00 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Br. (g) at equilibrium?
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