(i) The followig water gas shift reaction is an important industrial process for the production of hydrogen gas.
`CO(g)+H_(2)O(g)hArrCO_(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 2L flask, find out in which direction must the reaction proceed to reach equilibrium.
(ii) `2H_(2)O(g)hArr2H_(2)(g)+O_(2)(g)K_(c)=4.1xx10^(-48)" At 599 K"`
`N_(2)(g)+O_(2)hArr2NO(g)K_(c)=1xx10^(-30)" at 1000 K"`
Predict the extent of the above two reactions.

Explanation

(i) `CO(g)+H_(2)O(g)hArrCO_(2)(g)+H_(2)(g)`
Give `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)^(Deltang)`
`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`
`QgtK_(c)`, Hence, the reaction proceed in the reverse direction.
(ii) In the reactions, decomposition of water at 500 K and oxidation of nitrogen at 1000 K the value of `K_(c)` is very less `K_(c)lt10^*(-3)`. So reverse reaction is favoured.
`:.` Products `lt lt` reatants