Equilibrium constant, Kc for the reaction


Equilibrium constant, Kc for the reaction

$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longleftrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g})$ at $500 \mathrm{~K}$ is $0.061$

At a particular time, the analysis shows that composition of the reaction mixture is $3.0 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~N}_{2}, 2.0 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{H}_{2}$ and $0.5 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{NH}_{3}$. Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?


The given reaction is:

Now, we know that,




It is given that $K_{\mathrm{C}}=0.061$.

Since $Q_{C} \neq K_{C}$, the reaction is not at equilibrium.

Since $Q_{\mathrm{C}}

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