Water decomposes at `2300K`
`H_(2)O(g) rarr H_(2)(g)+(1)/(2)O_(2)(g)`
The percent of water decomposing at `2300K` and `1` bar is ____________ (Nearest integer).
Equilibrium constant for the reactions is `2times10^(-3)` at `2300K`.

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

The equilibrium constant for the reactions have been measured at 823 K. CoO(s) + H_(2)(g) hArr Co(s) + H_(2)O(g) , K = 67 CoO(s) + CO(g) hArr Co(s) + CO_(2) (g) , K = 490. From the data, calculate the equilibrium constant for the reaction. CO_(2)(g) +H_(2) (g) hArr CO(g) + H_(2)O (g)

The equilibrium constant for the following reactions at 1400 K are given. 2H_(2)O(g)hArr2H_(2)(g) + O_(2)(g) , K_(1)=2.1×x10^(-13) 2CO_(2)(g) hArr2CO(g)+O_(2)(g),K_(2) = 1.4 x× 10^(-12) Then, the equilibrium constant K for the reaction H_(2)(g) + CO_(2)(g)hArrCO(g) + H_(2)O(g) is

For the water gas reaction C(s)+H_(2)O(g)hArrCO(g)+H_(2)(g) The standard Gibb's energy of energy of reaction (at 1000K) is -8.1KJmol^(-1) . Value of equilibrium constant is -

For the process H_(2)O (l) (1"bar", 373 K) rarr H_(2)O (g) (1"bar", 373 K) , the correct set of thermodynamic parameters is:

For the reaction 2NO_(2)(g)+(1)/(2)O_(2)(g)hArrN_(2)O_(5)(g) if the equilibrium constant is K_(p) , then the equilibrium constant for the reaction 2N_(2)O_(5)(g)hArr4NO_(2)(g)+O_(2)(g) would be :

The equilibrium constants for the following reactions N_(2) (g) + 3H_(2)(g) hArr 2NH_(3) (g) N_(2) (g) + O_(2) (g) hArr 2NO(g) " and " H_(2)(g) +1//2 O_(2) (g) hArr H_(2)O (Ig) " are " K_(1) ,K_(2) " and " K_(3) respectively. The equilibrium constant (K) for the reaction 2NH_(3) (g) + 2^(1)//2) O_(2) (g) hArr 2NO(g) +3H_(2) O(I) " is "