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Question

Equilibrium constant, Kc for the reaction
N2(g)+3H2(g)2NH3(g) at 500K is 0.061
At a particular time, the analysis shows that composition of the reaction mixture is 3.0mol L1 N2,2.0mol L1 H2 and 0.5mol L1 NH3. Is the reaction at equilirbium? IF not in which direction does the reaction tend to proceed to reach equilibrium?

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Solution

The given reaction is:
N2(g)+3H2(g)2NH3(g)
At a particular time 3.0molL1 2.0molL1 0.5molL1
Now we know that,

QC=[NH3]2[N2][H2]3

QC=[0.5]2[3.0][2.0]3

QC=0.0104
it is given that, KC=0.061
since QCKC, the reaction not at equilibrium.
since QC<KC, the reaction will proceed in the forward direction to reach equilibrium.

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