At 2300 K the value of K of the following reaction is 1.5 x 10-3: N2(g)...

At 2300 K the value of K of the following reaction is 1.5 x 10^-3:

N₂(g) + O₂(g) ↔ 2NO(g)

At the instant when a reaction vessel at 2300K contains 0.50M N₂, 0.25M O₂, and 0.0042M NO, by calculation of the reaction quotient (Q), is the reaction mixture at equilibrium? If not, in which direction will the reaction proceed to reach equilibrium?

Expert Solution

Answer. for the given reaction rate constant at equilibrium is 1.5x10^-3. and the concentrations of reactants and products are given as [N₂]=0.50M,[O₂]=0.25 M, [NO]=0.0042M.

reaction quotient Q= [NO]²/[N₂][O₂] =(0.0042x0.0042) /0.50x0.25 =1.411x10^-4 it is less than the K value so the reaction is noy at equilibrium position and the reaction proceed in the forward direction to reach equilibrium.

queen_honey_blossom answered 2 years ago

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