question_answer

The equilibrium constant for the reactions (i) \[{{N}_{2}}+{{O}_{2}}\rightleftharpoons \,2NO\] and (ii) \[2NO+{{O}_{2}}\rightleftharpoons 2N{{O}_{2}}\] are \[{{K}_{1}}\] and \[{{K}_{2}}\] respectively, then what will be the equilibrium constant for the reaction \[{{N}_{2}}+2{{O}_{2}}\rightleftharpoons 2N{{O}_{2}}?\]

Answer:

                Adding eqns. (i) and (ii), we get the required equation. Thus, (i) and (ii) are the two steps of the required equation. Hence, for the required reaction, \[K={{K}_{1}}\times {{K}_{2}}\].