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At 1000 K , a sample of pure NO(2) gases...

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 :

A

(A) `0.03`

B

(B) `0.25`

C

(C) `0.025`

D

(D) `0.04`

Text Solution

Verified by Experts

The correct Answer is:
C
`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`
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