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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 L1 N2,2.0 mol L1 H2 and 0.5 mol L1 NH3. Is the reaction at equilibirium and if not in which direction does the reaction tend to proceed to reach equilibrium?

A
at equilibrium
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B
not at equilibrium, backwards shift
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C
not at equilibrium, forward shift
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D
can not be predicted
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Solution

The correct option is C not at equilibrium, forward shift
N2 (g)+3H2 (g)2NH3 (g)At t3 M2 M0.5 M
Q=[NH3]2[N2][H2]3
Q=0.5×0.53×23=13×8×4=196=0.0104

Q<K, the reaction will shift in forward direction.



Theory:

Kc (equilibrium constant) is directly proportional to product of concentration of products each raised to the corresponding stoichiometric coefficients and inversely proportional to product of concentration of reactants raised to the corresponding stoichiometric coefficients.
When,
Kc<103, the reaction will rarely proceed.
Kc>10+3, the reaction will proceed towards completion.
103<Kc<10+3, both the reactant and products are significant.

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