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At 457K NO2(g) was evacuated to a reaction chamber until the pressure was 0.0539 atm. When equilibrium was established: 2NO2(g)      ↔    2NO(g)      +     O2(g) the pressure inside the container was 0.0835 atm. (a)What is the partial pressures of the gases at equilibrium. (b) Calculate the equilibrium constant kp and kc at 457K.

At 457K NO2(g) was evacuated to a reaction chamber until the pressure was 0.0539 atm. When equilibrium was established: 2NO2(g)      ↔    2NO(g)      +     O2(g) the pressure inside the container was 0.0835 atm. (a)What is the partial pressures of the gases at equilibrium. (b) Calculate the equilibrium constant kp and kc at 457K.

Chemistry
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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  1. At 457K NO2(g) was evacuated to a reaction chamber until the pressure was 0.0539 atm. When equilibrium was established:

2NO2(g)      ↔    2NO(g)      +     O2(g)

the pressure inside the container was 0.0835 atm. (a)What is the partial pressures of the gases at equilibrium. (b) Calculate the equilibrium constant kp and kc at 457K.

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