Calculate the equilibrium constants `K_(p) and K_(c) ` for the reaction , `CO (g) + 1//2 O_(2) (g) hArr CO_(2)`
Given that the partial pressures at equilibrium in a vessel at 3000 K are `p_(co) = 0.4" atm ". p_(co_(2)) = 0.6 " atm "and p_(o_(2))= 0.2" atm"`

Answer

`K_(p)= 3.354, K_(c)= 52.64`

Explanation

`{:(,CO,+,1/2O_(2),hArr,CO_(2)),("At.eqm.",0*4 " atm",,0*2 " atm",,0*6 " atm"):}`
`K_(p) = (p_(CO_(2)))/(p_(CO) xx p_(O_(2))^(1//2))= (0*6)/(0*4 xx(0*2)^(1//2)) = 3*354`
`K_(p) = K_(c) (RT)Delta ^(n) or K_(c) = K_(p) //(RT)^(Delta n)= 3*354 //(0*0821 xx 3000)^(-1//2) = 52.64`