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Consider the following reaction at a high temperature. Br₂(g) = 2 Br (g) When 1.55 moles of Br₂ are put in a 0.720 L flask, 3.20 percent of the Br₂ undergoes dissociation. Calculate the equilibrium constant K for the reaction. Round your answer to 3 significant digits. Ke x X S

Consider the following reaction at a high temperature. Br₂(g) = 2 Br (g) When 1.55 moles of Br₂ are put in a 0.720 L flask, 3.20 percent of the Br₂ undergoes dissociation. Calculate the equilibrium constant K for the reaction. Round your answer to 3 significant digits. Ke x X S

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.31QP: You place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C...
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Consider the following reaction at a high temperature. Br₂(g) = 2 Br (g) C When 1.55 moles of Br₂ are put in a 0.720 L flask, 3.20 percent of the Br₂ undergoes dissociation. Calculate the equilibrium constant K for the reaction. Round your answer to 3 significant digits. с = x10 X Ś
Transcribed Image Text:Consider the following reaction at a high temperature. Br₂(g) = 2 Br (g) C When 1.55 moles of Br₂ are put in a 0.720 L flask, 3.20 percent of the Br₂ undergoes dissociation. Calculate the equilibrium constant K for the reaction. Round your answer to 3 significant digits. с = x10 X Ś
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