(`i`) The equilibrium `H_(2(g))+CO_(2(g))hArrH_(2)O_(2(g))+CO_((g))` is established in an evacuated vessel at `723 K` starting with `0.1 mol` of `H_(2)` and `0.2` mole of `CO_(2)`. If the equilibrium mixture contains `10` mole per cent of water vapour, calculate `K_(p)`, given that the equilibrium pressure is `0.5 atm`. Calculate the partial pressures of the component species and the volume of the container.
(`ii`) If now, into the flask, solid `CoO` and solid `Co` are introduced two new equilibrium are established.
`CoO_((s))+H_(2(g))hArrCo_((s))+H_(2)O_((g))`, `CoO_((s))+CO_((g))hArrCo_((g))+CO_(2(g))`
The new equilibrium mixture contains `30` mole per cent of water vapour. Calculate the equilibrium constants for the new equilibria.

Explanation

(`i`) `K_(p)=7.56xx10^(-2)`, `P'_(H_(2)O)=0.05atm`,
`P'_(H_(2))=0.1166atm`, `P'_(CO_(2))=0.2833atm`,
`V=35.6litre`, (`ii`) `K_(c_(1))=9.04`, `K_(c_(2))=110.1` ,