Calculating K from equilibrium concentrations and vice versa 8. At 298 K, the equilibrium constant for the following reaction is 6.50 x 10.³. 2 NOBr(g) 2 NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 10.5 L contains 9.496 mol NOBr(g) and 0.470 mol of NO, how many moles of Br2(g) are present at equilibrium?

Calculating K from equilibrium concentrations and vice versa 8. At 298 K, the equilibrium constant for the following reaction is 6.50 x 10.³. 2 NOBr(g) 2 NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 10.5 L contains 9.496 mol NOBr(g) and 0.470 mol of NO, how many moles of Br2(g) are present at equilibrium?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 60QRT

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