Consider the following system at equilibrium where AH° = 16.1 kJ/mol, and Kc = 6.50x10-3, at 298 K. 2 NOBr (g) = 2 NO (g) + Br₂ (g) When 0.19 moles of NOBr (g) are added to the equilibrium system at constant temperature: The value of Kel The value of Qc Кс. The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of NO will
Consider the following system at equilibrium where AH° = 16.1 kJ/mol, and Kc = 6.50x10-3, at 298 K. 2 NOBr (g) = 2 NO (g) + Br₂ (g) When 0.19 moles of NOBr (g) are added to the equilibrium system at constant temperature: The value of Kel The value of Qc Кс. The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of NO will
Chemistry: The Molecular Science
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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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Consider the following system at equilibrium where AH° = 16.1 kJ/mol, and Kc =
6.50x10-3, at 298 K.
2 NOBr (g) 2 NO (g) + Br₂ (g)
When 0.19 moles of NOBr (g) are added to the equilibrium system at constant
temperature:
The value of Kel
The value of Qcl
%
5
The reaction must
Orun in the forward direction to restablish equilibrium.
Orun
the reverse direction to restablish equilibrium.
O remain the same. It is already at equilibrium.
The concentration of NO will
✔
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