Recall from our discussion of the NO,-N2O4 equilibrium that NO, has a brownish color. At elevated temperatures, NO2 reacts with CO according to NO2(g) + CO(g) 2 NO(g) + CO2(g) The other three gases taking part in this reaction are color- less. When a gas mixture is prepared at 500 K, in which 3.4 atm is the initial partial pressure of both NO, and CO, and 1.4 atm is the partial pressure of both NO and CO2, the brown color of the mixture is observed to fade as the reaction progresses toward equilibrium. Give a condition that must be satisfied by the equilibrium constant K (for example, it must be greater than or smaller than a given number).
Recall from our discussion of the NO,-N2O4 equilibrium that NO, has a brownish color. At elevated temperatures, NO2 reacts with CO according to NO2(g) + CO(g) 2 NO(g) + CO2(g) The other three gases taking part in this reaction are color- less. When a gas mixture is prepared at 500 K, in which 3.4 atm is the initial partial pressure of both NO, and CO, and 1.4 atm is the partial pressure of both NO and CO2, the brown color of the mixture is observed to fade as the reaction progresses toward equilibrium. Give a condition that must be satisfied by the equilibrium constant K (for example, it must be greater than or smaller than a given number).
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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