9. Nitrogen monoxide is formed in automobile exhaust by the reaction of N2 and O2 from air, and produced by the following reaction: N2(g) + O2(g) <==> 2NO(g). The equilibrium constant for this reaction is 1.23 x 10-2 at 135°C. What is the direction of the reaction when a mixture that is 0.80 M N2, 0.60 M O2, and 0.10 M NO gets near equilibrium at 135°C?

9. Nitrogen monoxide is formed in automobile exhaust by the reaction of N2 and O2 from air, and produced by the following reaction: N2(g) + O2(g) <==> 2NO(g). The equilibrium constant for this reaction is 1.23 x 10-2 at 135°C. What is the direction of the reaction when a mixture that is 0.80 M N2, 0.60 M O2, and 0.10 M NO gets near equilibrium at 135°C?

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter9: Chemical Reactions

Section: Chapter Questions

Problem 9.76EP: Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the...

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