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Question
Equilibrium constant, Kc for the reaction
\[\ce{N2 (g) + 3H2 (g) ⇌ 2NH3 (g)}\] 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?
Solution
The given reaction is:
| N2(g) | + | 3H2(g) | ↔ | 2NH3(g) | |
| At a particular time | 3.0 mol L-1 | 2.0 mol L-1 | 0.5 mol L-1 |
Now, we know that,
`"Q"_"C" = ["NH"_3]^2/(["N"_2]["H"_2]^3)`
` =(0.5)^2/((3.0)(2.0)^3)`
= 0.0104
it is given that `"K"_"C"` = 0.061
Since `"Q"_"C" != "K"_"C"`, the reaction is not at equilibrium.
Since `"Q"_"C" < "K"_"C"`, the reaction will proceed in the forward direction to reach equilibrium.
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