At 1000 K , a sample of pure `NO_(2)` gases decomposes as :
`2NO_(2)(g)hArr2NO(g)+O_(2)(g)`
The equilibrium constant `K_(P)` is 156.25 atm .Analysis showns that the partial pressure of `O_(2)` is 0.25 atm at equilibrium .The parital pressure o f`NO_(2)` at equilibrium is :

Options

A. (A) `0.03`
B. (B) `0.25`
C. (C) `0.025`
D. (D) `0.04`

Answer

C

Explanation

`2NO_(2)hArr2NO(g)+O_(2)(g)`
` K_(p)=((P_(NO)^(2)(P_(O_2)))/((P_(NO_(2)))^(2)))`
given
`P_(O_(2))=0.25: P_(NO)=0.5`
`100=((0.5)^(2)(0.25))/(P_(NO_(2)^(2))`
`P_(NO_(2)^(2))= ((0.5)^(2)(0.25))/(100)`
`P_(NO_(2))=0.025`