The equilibrium constant `K_(p)` for the reaction
`H_(2)(g)+CO_(2)(g)hArrH_(2)(g)+CO(g)`
is 4.0 at `1660^(@)C` Inittally 0.80`H_(2) and 0.80 mole CO_(2)` are injecteed into a 5.0 litre flask what is the equilibrium concentraton of `CO_(2)(g)`?

The equilibrium constant K_(p) for the reaction H_(2)(g)+CO_(2)(g)hArrH_(2)O(g)+CO(g) is 4.0 at 1660^(@)C Initially 0.80 mole H_(2) and 0.80 mole CO_(2) are injected into a 5.0 litre flask. What is the equilibrium concentration of CO_(2)(g) ?

The equilibrium constant for the reaction , H_(2) (g) + CO_(2) (g) hArr H_(2) O (g) + CO (g) is 16 at 1000^(@) C . If 1.0 mole of H_(2) and 1.0 mole of CO_(2) are placed in one litre flask , the final equilibrium concentration of CO at 1000^(@) C is

The equilibrium constant for, H_2(g) +CO_2(g) hArr H_2O(g) + CO(g) is 1.80 at 1000^Oc . If 1.0 mole of H_2 and 1.0 mole of CO_2 are placed in one litre flask. What will be the final equilibrium concentration of CO at 1000^Oc ?

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

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

For the equilibrium H_(2)(g)+CO_(2)(g)hArr hArr H_(2)O(g)+CO(g), K_(c)=16 at 1000 K. If 1.0 mole of CO_(2) and 1.0 mole of H_(2) are taken in a l L flask, the final equilibrium concentration of CO at 1000 K will be