question_answer

2 mol of \[{{N}_{2}}\]is mixed with 6 mol of \[{{H}_{2}}\] in a closed vessel of one litre capacity if 50% of \[{{N}_{2}}\] is converted into \[N{{H}_{3}}\]  at equilibrium, the ratio of \[\frac{{{K}_{f}}}{{{K}_{b}}}\] (rate constants) value of \[{{K}_{c}}\] for the reaction\[{{K}_{2(g)}}+3{{H}_{2(g)}}2N{{H}_{3(g)}}\] is :

A)  \[\frac{4}{27}\]                        

B)  \[\frac{27}{4}\]

C)  \[\frac{1}{27}\]                        

D)  24