At 2000 K the equilibrium constant for the formation of NO(g) is 4.0 x 10-4 N2(g) + O2(g) -> <- 2NO(g) You have a flask in which, at 2000 K, the concentration of N2 is 0.50 M, that of O2 is 0.25 M, and that of NO is 4.2 x 10-3 M. Which direction will the reaction proceed to achieve equilibrium?
At 2000 K the equilibrium constant for the formation of NO(g) is 4.0 x 10-4 N2(g) + O2(g) -> <- 2NO(g) You have a flask in which, at 2000 K, the concentration of N2 is 0.50 M, that of O2 is 0.25 M, and that of NO is 4.2 x 10-3 M. Which direction will the reaction proceed to achieve equilibrium?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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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At 2000 K the equilibrium constant for the formation of NO(g) is 4.0 x 10-4
N2(g) + O2(g) -> <- 2NO(g)
You have a flask in which, at 2000 K, the concentration of N2 is 0.50 M, that of O2 is 0.25 M, and that of NO is 4.2 x 10-3 M. Which direction will the reaction proceed to achieve equilibrium?
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