Question:
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 N₂, 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?

Answer:

The given reaction is:

N₂ (g) + 3H₂ (g) ↔ 2NH₃ (g)

at a particular time: 3.0molL^-1 2.0 molL^-1 0.5molL^-1

Now, we know that,

Qc = [NH₃]² / [N₂][H₂]³

= (0.5)² / (3.0)(2.0)³

= 0.0104

It is given that K_c = 0.061

Since,Qc ≠ Kc, the reaction mixture is not at equilibrium.

Again, Qc < Kc, the reaction will proceed in the forward direction to reach equilibrium.

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