The following euilibrium constants are given:
`N_2+3H_2 `H_2+1/2O^2 The equilibrium constant for the oxidation of 2 mol of `NH_3` to give NO is-

Options

A. `K_1xx(K_2)/(K_3)`
B. `K_2xx(K_3^3)/(K_1)`
C. `K_2xx(K_3^2)/(K_1)`
D. `K_2^2xx(K_3)/(K_1)`

Explanation

`2NH_3 `N_2+O_2 `3H_2+3/2O_2 `2NH_3+5/2O_2 The equilibrium constant of the reaction is the product of the equilibrium constant of (1)(2) and (3) i.e. `(K_2K_3^3)/(K_1)`