Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
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Question
![Identify the equilibrium expression for the reaction CH₂CHO(g) ➡ CH₂(g) + CO(g).
For the reaction 2 NO + O₂ <--> 2 NO₂ the value of Kp = 2.3 x 108 at 25°C. What is the value of
the reverse rate constant?
For the reaction: 2 NO2(g) --> N₂O4(g)
3.00M NO₂ gas is placed in a flask and allowed to come to equilibrium according to the equation.
Calculate the equilibrium to 3 sig figs of concentration of N₂O4 if Kc=9.3 x 10-7](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffc7deb2c-0862-415e-88b2-023e0d274874%2F0d2fd605-f1e0-4357-b6b5-4d186f29f5ca%2Fj6igbe_processed.png&w=3840&q=75)
Transcribed Image Text:Identify the equilibrium expression for the reaction CH₂CHO(g) ➡ CH₂(g) + CO(g).
For the reaction 2 NO + O₂ <--> 2 NO₂ the value of Kp = 2.3 x 108 at 25°C. What is the value of
the reverse rate constant?
For the reaction: 2 NO2(g) --> N₂O4(g)
3.00M NO₂ gas is placed in a flask and allowed to come to equilibrium according to the equation.
Calculate the equilibrium to 3 sig figs of concentration of N₂O4 if Kc=9.3 x 10-7
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