The following water gas shift reaction is an important industrial process for the production of hydrogen gas .
`CO (g) + H_(2) O(g) hArr CO_(2) (g) + H_(2) (g)`
At a given temperature `K_(p) = 2.7` . If `0.13` mol of CO , 0.56 mol of water , 0.78 mol of `CO_(2)` and 0.28 mol of `H_2` are introduced into a 21 . flask , find out in which direction must the reaction proceed to reach equilibrium .

Explanation

`CO (g) + H_2 O (g) hArr CO_(2) (g) + H_(2) (g)`
Given `" " K_(p) = 2.7`
`[CO] = 0.13` mol . `[H_(2)O] = 0.56` mol
`[CO_(2)] = 0.78` mol , `[H_(2)] = 0.28` mol
` V = 2L `
`K_p = K_(C) (RT)^(Delta n_(g))`
`2.7 = K_(C) (RT)^(0)`
`K_(C) = 2.7`
`Q_(C) = ([CO_(2)] [H_(2)])/([CO] [H_(2)O]) = (((0.78)/(2)) ((0.28)/(2)))/(((0.13)/(2)) ((0.56)/(2)))`
Q = 3
`Q gt K_(C)` , Hence , the reaction proceed in the reverse direction