34. At 25°C, the equilibrium constant for the reaction 2 NO2(g) 2 2 NO(g) + O2(g) is 5.9 x 10-13. Suppose a container is filled with nitrogen dioxide at an initial partial pressure of 0.89 atm. Calculate the partial pressures of all three gases after equilibrium is reached at this temperature.
34. At 25°C, the equilibrium constant for the reaction 2 NO2(g) 2 2 NO(g) + O2(g) is 5.9 x 10-13. Suppose a container is filled with nitrogen dioxide at an initial partial pressure of 0.89 atm. Calculate the partial pressures of all three gases after equilibrium is reached at this temperature.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 33P
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Question
![34. At 25°C, the equilibrium constant for the reaction
2 NO2(g)
2 NO(g) + O2(g)
is 5.9 x 10-13. Suppose a container is filled with nitrogen
dioxide at an initial partial pressure of 0.89 atm. Calculate
the partial pressures of all three gases after equilibrium is
reached at this temperature.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8b661251-6f9a-4090-a1f5-56e54f1837ca%2F2f095d2d-0dfe-4cc3-bf1a-79db956eba8d%2F0kgbgl_processed.png&w=3840&q=75)
Transcribed Image Text:34. At 25°C, the equilibrium constant for the reaction
2 NO2(g)
2 NO(g) + O2(g)
is 5.9 x 10-13. Suppose a container is filled with nitrogen
dioxide at an initial partial pressure of 0.89 atm. Calculate
the partial pressures of all three gases after equilibrium is
reached at this temperature.
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