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Question

Equilibrium constant, KC for the reaction at 500K is 0.061. N2(g)+3H2(g)2NH3(g). At a particular time, the analysis shows that composition of the reaction mixture is 3.0 molL1 N2, 2.0 molL1 H2 and 0.5 molL1 NH3. Is the reaction at equilibrium 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, backward 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
The equilibrium reaction is shown below:
N2(g)+3H2(g)2NH3(g)
The concentrations of nitrogen, hydrogen and ammonia are 3M, 2M and 0.5M respectively.
The expression for the reaction quotient is Q=[NH3]2[N2][H2]=0.5×0.53×23=13×8=0.0104.
The value of the reaction quotient is smaller than the value of the equilibrium constant.

Hence, the reaction will progress in the forward direction so that the equilibrium is achieved. The reaction is not at equilibrium.

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