The equilibrium constant for the reaction `CO(g)+H_(2)O(g)hArrCO_(2)(g)+H_(2)(g) is 5` how many moles of `CO_(2)` must be added to 1 litre container alrady containing 3 moles each of CO and `H_(2)O` to make 2 M equilibrium conentration of CO?

The equilibrium constant for the reaction CO_((g)) + H_(2) O_((g)) hArr CO_(2(g)) + H_(2(g)) is 5. How many moles of CO_(2) must be added to I lit container already containing 3 moles of each of CO and H_(2) O to make 2M equilibrium concentration of CO ?

Write the equilibrium constant of the reaction C(s)+H_(2)O(g)hArrCO(g)+H_(2)(g)

Write the equilibrium constant of the reaction C(s)+H_(2)O(g)hArrCO(g)+H_(2)(g)

At a certain temperature , the equilibrium constant (K_(c)) is 4//9 for the reaction : CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) If we take 10 mole of each of the four gases in a one - litre container, what would be the equilibrium mole percent of H_(2)(g) ?

At a certain temperature , the equilibrium constant (K_(c)) is 4//9 for the reaction : CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) If we take 10 mole of each of the four gases in a one - litre container, what would be the equilibrium mole percent of H_(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

For the reaction, CO(g)+H_(2)O(g)hArrCO_(2)(g)+H_(2)(g) , at a given temperature, the equilibrium amount of CO_(2)(g) can be increased by