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Equilibrium constant, KC for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) at 500 K is 0.061. At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L-1, 2.0 mol L-1 H2 and 0.5 mol L-1 NH3. Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

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[N2] = 3.0 mol L-1

[H2] = 2.0 mol L-1

[NH3] = 0.50 mol L-1

N2(g) + 3H2(g) ⇌ 2NH3

QC\(\frac{[NH_3]^2}{[N_2][H_2]^3}\) = \(\frac{(0.50)^2}{3 \times (2)^3}\) = 0.0104

Thus at the stage of the reaction QC < KC

Therefore, the reaction is not at equilibrium. The reaction proceeds to form more products.

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