An equilibrium mixture
`CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g)`
present in a vessel of one litre capacity at `815^(@)C` was found by analysis to contain `0.4` mol of CO, `0.3` mol of `H_(2)O, 0.2` mol of `CO_(2)` and `0.6` mol of `H_(2)`.
a. Calculate `K_(c)`
b. If it is derived to increase the concentration of CO to `0.6` mol by adding `CO_(2)` to the vessel, how many moles must be addes into equilibrium mixture at constant temperature in order to get this change?

Explanation

`{:(,CO(g)+, H_2O(g) hArr , CO_2(g)+, H_2(g)),("Mole at equilibrium" , 0.4,0.3,0.2,0.6):}`
`therefore K_C=([CO_2][H_2])/([CO][H_2O])=(0.2xx0.6)/(0.4xx0.3)=1`
( ? `Deltan=0` , `therefore` Volume terms are not needed. )