Answer:
Information shadow:
Reaction: \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons
2N{{H}_{3}}(g)\]
\[{{K}_{c}}=0.061at500K\]
Composition
of reaction mixture:
\[[{{N}_{2}}]=3mol{{L}^{-1}};[{{H}_{2}}]=2mol{{L}^{-1}},[N{{H}_{3}}]=0.5mol\,{{L}^{-1}}\]
Problem
solving strategy:
Reaction
quotient Q can be calculated as:
\[Q=\frac{{{[N{{H}_{3}}]}^{2}}}{[{{N}_{2}}]{{[{{H}_{2}}]}^{3}}}\]
Comparison
of Q with K will decide whether the reaction is at equilibrium or not.
Working
it out:
\[Q=\frac{{{[0.5]}^{2}}}{3\times {{(2)}^{3}}}=\frac{0.25}{24}=0.01\]
\[Q\ne K;\]the
reaction is not at equilibrium.
\[Q>{{K}_{c}};\]the net reaction will be towards right.
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