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?

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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 1 year ago

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