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4 HBr(g) + O2(g) 2 Br(g) + 2H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition: compound pressure at equilibrium HBr 70.2 atm 02 49.8 atm Br₂ 46.5 atm H₂O 75.7 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K-0 =

4 HBr(g) + O2(g) 2 Br(g) + 2H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition: compound pressure at equilibrium HBr 70.2 atm 02 49.8 atm Br₂ 46.5 atm H₂O 75.7 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K-0 =

Chemistry: Principles and Reactions
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 85QAP
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Hydrogen bromide and oxygen react to form bromine and water, like this: 4 HBr(g) + O2(g) 2 Bг2(g) + 2 H₂O(g) - Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition: compound pressure at equilibrium HBr 70.2 atm 0, 49.8 atm Br2 46.5 atm H₂O 75.7 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. = P x10
Transcribed Image Text:Hydrogen bromide and oxygen react to form bromine and water, like this: 4 HBr(g) + O2(g) 2 Bг2(g) + 2 H₂O(g) - Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition: compound pressure at equilibrium HBr 70.2 atm 0, 49.8 atm Br2 46.5 atm H₂O 75.7 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. = P x10
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