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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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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