The equilibrium mixture for
`2SO_(2)(g) +O_(2)(g) hArr 2SO_(3)(g)`
present in `1 L` vessel at `600^(@)C` contains `0.50, 0.12`, and `5.0` moles of `SO_(2), O_(2)`, and `SO_(3)` respectively.
a. Calculate `K_(c)` for the given change at `600^(@)C`.
b. Also calculate `K_(p)`.
c. How many moles of `O_(2)` must be forced into the equilibrium vessel at `600^(@)C` in order to increase the concentration of `SO_(3)` to `5.2` mol?

Explanation

`{:(,2SO_2(g)+ , O_2(g) hArr , 2SO_3(g)),("Equi.conc.", 0.5,0.12,5.0):}`
`K_c=[SO_3]^2/([SO_2]^2[O_2])=(5.0)^2/((0.5)^2(0.12))=833.3 "mol"^(-1) L` .
`K_p=K_c(RT)^(Deltan)`
`K_p=833.3xx(0.082xx873)^(-1)=11.64 "atm"^(-1)`