Dihydrogen gas used in Haber's process is produced by reacting methane from natural gas with high temperature steam. The first stage of the two `2` stage reaction involves the formation of `CO` and `H_(2)`. In second stage, `CO` formed in first stage is reacted with more steam in water gas shift reaction,
`CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g)`
If a reaction vessel at `400^(@)C` is charged with an equimolar mixture of `CO` and steam such that `p_(CO)=p_(H_(2)O)=4.0` bar, what will be the partial pressure of `H_(2)` at equilibrium? `K_(p)=0.1` at `400^(@)C`.

Explanation

Let the partial pressure of hydrogen `(H_(2))` at equilibrium point =p bar

`K_(p) =(Pco_(2)xxP_(H_(2)))/("Pco"xx P_(H_(2)O))" or " 0.1 =((p " bar ")xx(p " bar "))/((4-p) " bar " xx(4-p) " bar ")`
`(P^(2))/((4-p)^(2)) =0.1 " or " (P)/((4-P)) =(0.1)^(1//2) =0.316`
`P= 0.316 (4 -P) " or " P 1.264 -0.316 p`
`1.316 p =1.264 " or " p=(1.264)/(1.316) =0.96 " bar "`