Consider the following system at equilibrium where AH° = 16.1 kJ, and Ke = 6.50x10-3, at 298 K.%3D2NOBR(g)2 2NO(g) + Br2(g)When 0.13 moles of NO(g) are removed from the equilibrium system at constant temperature:The value of KeThe value of Qc8 Kc.The reaction mustOrun in the forward direction to restablish equilibrium.run in the reverse direction to restablish equilibrium.remain the same. It is already at equilibrium.The concentration of Br2 willSubmit AnswerTry Another Version1 item attempt remaining

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Consider the following system at equilibrium where AH° = 16.1 kJ, and Ke = 6.50x10-3, at 298 K. %3D 2NOBR(g) 2 2NO(g) + Br2(g) When 0.13 moles of NO(g) are removed from the equilibrium system at constant temperature: The value of Ke The value of Qc Ke. The reaction must Orun in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of Br2 will

Consider the following system at equilibrium where AH° = 16.1 kJ, and Ke = 6.50x10-3, at 298 K. %3D 2NOBR(g) 2 2NO(g) + Br2(g) When 0.13 moles of NO(g) are removed from the equilibrium system at constant temperature: The value of Ke The value of Qc Ke. The reaction must Orun in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of Br2 will

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 61QRT

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