Consider the following system at equilibrium where AH° = 16.1 kJ, and Kc = 6.50×10-3, at 298 К. 2NOBr(g)=2NO(g) + Br2(g) When 0.26 moles of NO(g) are removed from the equilibrium system at constant temperature: The value of K The value of Qc Kc. The reaction must O run in the forward direction to restablish equilibrium. O run in the reverse direction to restablish equilibrium. O 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 Kc = 6.50×10-3, at 298 К. 2NOBr(g)=2NO(g) + Br2(g) When 0.26 moles of NO(g) are removed from the equilibrium system at constant temperature: The value of K The value of Qc Kc. The reaction must O run in the forward direction to restablish equilibrium. O run in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of Br2 will
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 54QAP: Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When...
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