The following equilibrium constants are given:
`N_(2) + 3H_(2) <=> 2NH_(3) , K_(1)`
`N_(2) + O_(2) <=> 2NO , K_(2)`
`H_(2) + 1//2 O_(2) <=> H_(2)O , K_(3)`
The equilibrium constant for the oxidaton of 2 mole `NH_(3)` by oxygen to give `NO` is

The following equilibrium constants are given : N_(2) + 3 H_(3) hArr 2 NH_(3) , K_(1) N_(2) + O_(2) hArr 2 NO , K_(2) H_(2) + 1/2 O_(2) hArr H_(2) O , K_(3) The equilibrium constant for the oxidation of NH_(3) by oxygen to give NO is :

The following equilibrium constants are given : N_(2)+3H_(2)hArr 2NH_(3), K_(1) N_(2)+O_(2)hArr 2NO, K_(2) H_(2)+(1)/(2)O_(2)hArr H_(2)O, K_(3) The equilibrium constant for the oxidation of NH_(3) by oxygen to give NO is :

The following equilibrium constants are given N_2+3H_2 harr 2NH_3,K_1 N_2+O_2 harr 2NO , K_2 H_2+1/2 O_2 harr H_2O , K_3 The equlibrium constant for the oxidation of NH_3 by oxygen to given NO is

The following equilibrium constants are given N_2+3H_2 harr 2NH_3,K_1 N_2+O_2 harr 2NO , K_2 H_2+1/2 O_2 harr H_2O , K_3 The equlibrium constant for the oxidation of NH_3 by oxygen to given NO is

The equilibrium constants of the following are - N_(2) + 3H_(2) hArr 2 NH_(3) , K_(1) " " N_(2) + O_(2) hArr 2 NO , K_(2) H_(2) + (1)/(2) O_(2) to H_(2)O , K_(3) The equilibrium constant (K) of the reaction : 2NH_(3) + (5)/(2) O_(2) overset(K)(hArr) 2 NO + 3 H_(2) O , will be -

The following equilibria and their equilibrium constants are given N_(2)+3H_(2) iff 2NH_(3)(K_(1)) N_(2)+O_(2) iff 2NO(K_(2)) H_(2)+1/2O_(2) iff H_(2)O(K_(3)) Therefore, the equilibrium constant of the reaction 2NH_(3)+5/2O_(2) iff 2NO+3H_(2)O in terms of K_(1), K_(2) and K_(3) is :

The following equilibria are given by : N_(2)+3H_(2) hArr 2NH_(3), K_(1) N_(2)+O_(2) hArr 2NO,K_(2) H_(2)+(1)/(2)O_(2) hArr H_(2)O, K_(3) The equilibrium constant of the reaction 2NH_(3)+(5)/(2)O_(2)hArr 2NO +3H_(2)O in terms of K_(1) , K_(2) and K_(3) is