A) The reaction is at equilibrium.
B) The reaction goes in the direction of reactants.
C) The reaction goes in the direction of product.
D) None of these.
Correct Answer: B
Solution :
[b]: \[{{N}_{2(g)}}+3{{H}_{2(g)}}2N{{H}_{3(g)}}\] \[{{Q}_{c}}=\frac{{{[N{{H}_{3}}]}^{2}}}{[{{N}_{2}}]{{[{{H}_{2}}]}^{3}}}\] Given, \[[N{{H}_{2}}]=\frac{8.13}{20}M=0.4065M;\] \[[{{N}_{2}}]=\frac{1.57}{20}M=0.0785M\] \[[{{H}_{2}}]=\frac{1.92}{20}M=0.096M\] \[{{Q}_{c}}=\frac{{{(0.4065M)}^{2}}}{(0.0785M){{(0.096M)}^{3}}}=2.379\times {{10}^{3}}{{M}^{-2}}\] \[{{Q}_{c}}\ne {{K}_{c}}\] , so the reaction is not in equilibrium. \[{{Q}_{c}}>{{K}_{c}}\] it indicates that the reaction will proceed in the direction of reactants.You need to login to perform this action.
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