Reaction `2BaO_(2)(s)hArr2BaO(s) + O_(2)(g), Delta H = +ve`. At equilibrium condition, pressure of `O_(2)` is depended on:

H_(2) O(l) hArr H_(2) O_((s)) , Delta H = - q application of pressure on this equilibrium

In the reaction 2BaO_(2) rarr 2BaO +O_(2) the oxidation number of Barium

The equilibrium constant of the following reactions at 400 K are given: 2H_(2)O(g) hArr 2H_(2)(g)+O_(2)(g), K_(1)=3.0xx10^(-13) 2CO_(2)(g) hArr 2CO(g)+O_(2)(g), K_(2)=2xx10^(-12) Then, the equilibrium constant K for the reaction H_(2)(g)+CO_(2)(g) hArr CO(g)+H_(2)O(g) is

For the equilibrium 2H_(2)O(g) hArr 2H_(2)(g)+O_(2)(g) , equilibrium constant is K_(1) For the equilibrium 2CO_(2)hArr 2CO(g)+O_(2)(g) , equilibrium constant is K_(2) The equilibrium constant for : CO_(2)(g)+H_(2)(g)hArr CO(s)+H_(2)O(g) is :

2Cl(s)+O_(2)(g)hArr2CO(g) DeltaHlt0 . What is the equilibrium expression for the reaction represented by the equation above?