1. The following reaction has been studied at 230 °C: 2NO(g) + O₂(g) = 2NO2(g) The reaction was allowed to reach equilibrium and the concentrations are: [NO] = 0.0452 M, [0₂] = 0.127 M, [NO₂] = 15.5 M. a) Write the equilibrium equation, K, and calculate the equilibrium constant. b) Express the equilibrium equation as K, and calculate K, (where Kp = Kc(RT), R is the gas constant, 0.0821 L*atm/K*mol, T is temperature in K).

1. The following reaction has been studied at 230 °C: 2NO(g) + O₂(g) = 2NO2(g) The reaction was allowed to reach equilibrium and the concentrations are: [NO] = 0.0452 M, [0₂] = 0.127 M, [NO₂] = 15.5 M. a) Write the equilibrium equation, K, and calculate the equilibrium constant. b) Express the equilibrium equation as K, and calculate K, (where Kp = Kc(RT), R is the gas constant, 0.0821 Latm/Kmol, T is temperature in K).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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