Carbonyl bromide, COBr2, decomposes to CO and Br2 with an equilibrium constant, Kc, of 1.90 x 10-6 at 73° C : COBr2 (g) —> CO(g) + Br2 (g) If 0.025 mol of COBr2 is placed in a 5.O L flask to decompose, what are the concentrations of all species at equilibrium?

Chemistry: Principles and Practice
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.51QE
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Carbonyl bromide, COBr2, decomposes to CO and Br2 with an equilibrium constant, Kc, of 1.90 x 10-6 at 73° C : COBr2 (g) —> CO(g) + Br2 (g) If 0.025 mol of COBr2 is placed in a 5.O L flask to decompose, what are the concentrations of all species at equilibrium?
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