Answer:
We know,
\[\Delta G=\Delta
{{G}^{o}}+RT{{\log }_{e}}Q\,\,\,\,\,\,\,\,\,\,\,\,.....(i)\]
where\[\Delta G\] = Free energy
change
\[\Delta {{G}^{o}}\] = Standard
free energy change
Q = Reaction Quotient
At equilibrium, \[\Delta G=0\]
and Q = K (equilibrium constant)
\[\therefore \]\[\Delta
{{G}^{o}}=-RT{{\log }_{e}}K\,\,\,\,\,\,\,\,\,\,\,......(ii)\]
from eqns. (i) and (ii)
\[\Delta G=-RT{{\log
}_{e}}K+RT{{\log }_{e}}Q\]
\[\Delta G=RT{{\log }_{e}}\left(
\frac{Q}{K} \right)\]
·
When Q < K, \[\Delta G\] will be negative and reaction will spontaneous
in forward direction.
·
When Q = K, \[\Delta G=0\]and reaction will be at equilibrium.
When pressure is increased, the given reaction will proceed
in forward direction where the number of gas moles are decreasing.
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