`K_(1)` and `K_(2)` are equilibrium constants for reaction (i) and (ii)
`N_(2)(g)+O_(2)(g) hArr 2NO(g)` …(i)
`NO(g) hArr 1//2 N_(2)(g)+1//2O_(2)(g)` …(ii)
then,

For the gaseous reactions (I) and (II) the equilibrium constants are X and Y respectively. I. (1)/(2)N_(2)(g) + O_(2) (g) hArr NO_(2)(g) (II) 2NO_(2)(g) hArr N_(2)O_(4) (g) Using the above reactions the equilibrium constant Z for the reaction (III) given below is III. N_(2)O_(4)(g) hArr N_(2)(g) + 2O_(2) (g)

If the equilibrium constant for N_(2) (g) + O_(2)(g) hArr 2NO(g) is K , the equilibrium " constant for " 1/2 N_(2) (g) +1/2 O_(2) (g) hArr NO (g) will be

If the equilibrium constant for N_(2) (g) + O_(2)(g) hArr 2NO(g) is K , the equilibrium " constant for " 1/2 N_(2) (g) +1/2 O_(2) (g) hArr NO (g) will be

Write the equilibrium constant expressions for the following reactions : (i) 1/2N_2(g)+3/2H_2(g) hArr NH_3(g) (ii) 2H_2O(g) hArr 2H_2(g)+O_2(g)