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Question

A mixture of 1.57 moles of N2,1.92 moles of H2 and 8.13 moles of NH3 is introduced into a 20L reaction vessel at 500K. At this temperature, the equilibrium constant, Kc for the reaction, N2(g)+3H2(g)2NH3(g)is1.7×102. What is the direction of the net reaction?

A
Forward
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B
Backward
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C
At equilibrium
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D
Data is insufficient
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Solution

The correct option is B Backward
The given reaction is :-
N2+3H22NH3
Now, we have
QC=[NH3]2[N2][H2]3
=(8.1320)2(1.5720)×(1.9220)3 (concentration=no.ofmolesvolume)
=20×8.13×8.13×201.57×1.92×1.92×1.92
=2.38×103
Given, KC=1.7×102
Now, QCKC, so the reaction is not at equilibrium.
Now, QC>KC, so the reaction will go towards backward direction.

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