(1) \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g),{{K}_{1}}\](2) \[{{N}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2NO(g),{{K}_{2}}\](3) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\rightleftharpoons {{H}_{2}}O(g),{{K}_{3}}\]The equation for the equilibrium constant of the reaction\[2N{{H}_{3}}(g)+\frac{5}{2}{{O}_{2}}(g)\rightleftharpoons 2NO(g)+3{{H}_{2}}O(g),\]\[({{K}_{4}})\] in terms of \[{{K}_{1}},{{K}_{2}}\] and\[~{{K}_{3}}\] is:

• A. \[\frac{{{K}_{1}}.{{K}_{2}}}{{{K}_{3}}}\]
• B. \[\frac{{{K}_{1}}.K_{3}^{2}}{{{K}_{2}}}\]
• C. \[{{K}_{1}}{{K}_{2}}{{K}_{3}}\]                   
• D. \[\frac{{{K}_{2}}.K_{3}^{3}}{{{K}_{1}}}\]