At `298 K`, the equilibrium between `N_(2)O_(4)` and `NO_(2)` is represented as : `N_(2)O_(4(g))hArr2NO_(2(g))`. If the total pressure of the equilibrium mixture is `P` and the degree of dissociation of `N_(2)O_(4(g))` at `298 K` is `x`, the partial pressure of `NO_(2(g))` under these conditions is:

Options

A. `((2x)/(1+x))P`
B. `2xP`
C. `((2x)/(1-x))P`
D. `(2)/(3)xP`

Explanation

`underset((1-x))underset(1)(N_(2)O_(4))hArrunderset(2x)underset(0)(2NO_(2))`
`P'_(NO_(2))=P_("total")xx"Mole fraction of" NO_(2)`
`=(P*2x)/((1+x))`