NO2 (g) = 2 N204 (g) (brown) (colorless) When the temperature decreases, the color of the equilibrium mixture gets lighter. Is reaction exothermic or endothermic? What will happen to the value of the equilibrium constant, K, if the temperature of th reaction is increased?
NO2 (g) = 2 N204 (g) (brown) (colorless) When the temperature decreases, the color of the equilibrium mixture gets lighter. Is reaction exothermic or endothermic? What will happen to the value of the equilibrium constant, K, if the temperature of th reaction is increased?
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...
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