The following reactions have the indicated equilibrium constants at a particular temperature: -25 N2(g) + O2(g) = 2NO(g) K = 4.3 x 10 2NO(g) + 02(g)=2NO2(g) K = 6.4 x 10° Determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4NO(g) = N2g) + 2NO2(g) x 10 (b) 4NO,(g) = 2N,(g) + 402(g) x 10 (c) 2NO(g) + 2N02(g) = 302(g) + 2N½(g) x 10

The following reactions have the indicated equilibrium constants at a particular temperature: -25 N2(g) + O2(g) = 2NO(g) K = 4.3 x 10 2NO(g) + 02(g)=2NO2(g) K = 6.4 x 10° Determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4NO(g) = N2g) + 2NO2(g) x 10 (b) 4NO,(g) = 2N,(g) + 402(g) x 10 (c) 2NO(g) + 2N02(g) = 302(g) + 2N½(g) x 10

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.2QE: Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium...

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