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For the reaction : CO(g)+1//2O(2)(g)...

For the reaction :
`CO(g)+1//2O_(2)(g)hArr CO_(2)(g)`
the partial pressures are :
`p(O_(2))=0.24` atm, `p(CO)=0.4` atm and `p(CO)=0.04` atm. The equilibrium constant `K_(p)` is :

A

`0.3`

B

`3.0`

C

`9.0`

D

`0.03`

Text Solution

Verified by Experts

The correct Answer is:
B
`K_(p)=((p CO_(2)))/(p(CO)xx [p(O_(2))]^(1//2))`
`=(0.24)/(0.4xx(0.04)^(1//2))=3.0`
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