(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.

(i) The followig water gas shift reaction is an important industrial p

1.	(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.
Answer» Solution :(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