The equilibrium constant `(K_c)` for the reaction `N_2(g)+O_2(g)to2NO(g)` at temperature T is `4xx10^(-4)` The value of `K_c` for `NO(g)to1/2N_s(g)+1/2O_2(g)` at the same temperature is

Options

A. `2.5xx10^2`
B. `4xx10^(-4)`
C. 50
D. 0.02

Explanation

`N_2(g)+O_2(g)to2NO(g)`....[i] `K_c=4XX10^(-4)`
Multiplying the equation [i] by `1/2` we get
`1/2N_2(g)+1/2O_2(g)toNO(g)`
`K_c^'=sqrt(K_c)=sqrt(4xx10^(-4)=2xx10^(-2)`
Reversing the equation [ii] we get
`NO(g)to1/2N_2(g)+1/2O_2(g)`
`K_c^"=1/(K_c^')=1/(2xx10^(-2))=50.0`