For the reaction
`C_((s))+CO_(2(g))hArr2CO_((g))K_(p)=63` atm at 1000 K.If at equilibrium partial pressure of CO is then times that of `CO_(2)`, then the total pressure of the gases at equilibrium is …….atm

Answer

`6.93`

Explanation

`C_((s))+CO_(2(g))hArr2CO_((g)),K_(p)=63`atm
`K_(p)=((P_(co))^(2))/(P_(co_(2)))=63`
Now `P_(co)=10xxP_(CO_(2))` at equilibrium
`:.634=((10xxP_(CO_(2)))^(2))/(P_(CO_(2)))`
`:.P_(CO_(2))=0.63` atm
`:.P_(CO)=10xx0.63=6.30` atm
`:.` Total pressure` =P_(CO_(2))+P_(CO)`
`=0.63+6.30`
`=6.93` atm