In a 20 litre vessel at 300 K initially, 1 mole of `CO, H_(2)O, CO_(2)` are present, then for the equilibrium of `CO+H_(2)OhArr CO_(2)+H_(2)` which of the following is true?

In a 20 litre vessel initially each have 1-1 mole. CO,H_(2)OCO_(2) is present, then for the equilibrium of CO+H_(2)OhArrCO_(2)+H_(2) following is true:

K_(p) for the reaction : CO_(2)(g)+H_(2)(g) hArr CO(g)+H_(2)O(g) is found to be 16 at a given temperature. Originally equal number of moles of H_(2) and CO_(2)(g) were placed in the flask. At equilibrium, the pressure of H_(2) is 1.20 atm. What is the partial presure of CO_(2) and H_(2)O ?

CO_(2)+ H_(2)O to ………….

At a given temperature, Ke is 4 for the reaction H_(2(g)) + CO_(2(g)) hArr H_(2)O_((g)) + CO_((g)) . Initially 0.6 moles each of H_(2) and CO_(2) are taken in 1lit flask. The equilibrium concentration of H_(2) O_((g)) is

( 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.

The value of K for H_(2)(g)+CO_(2)(g)hArr H_(2)O(g)+CO(g) is 1.80 at 1000^(@)C . If 1.0 mole of each H_(2) and CO_(2) placed in 1 litre flask, the final equilibrium concentration of CO at 1000^(@)C will be

The value of K for H_(2)(g)+CO_(2)(g)hArr H_(2)O(g)+CO(g) is 1.80 at 1000^(@)C . If 1.0 mole of each H_(2) and CO_(2) placed in 1 litre flask, the final equilibrium concentration of CO at 1000^(@)C will be