For the water gas reaction,
`C(s) +H_(2)O(g) hArr CO(g)+H_(2)(g)`
the standard Gobbs free energy of reaction (at `1000K)` is `-8.1 kJ mol^(-1)`. Calculate its equilibrium constant.

For the water gas reaction: C(s) +H_(2)O(g) hArr CO(g) +H_(2)(g) the standard Gibbs enegry for the reaction at 1000K is -8.1 kJ mol^(-1) . Calculate its equilibriu constant.

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 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 a water gas reaction, C_((s)) + H_(2)O_((g)) hArr CO_((g)) + H_(2(g)) at 1000 K, the standard Gibb's energy change is -8.1 kJ mol^(-1) . Calculate the value of equilibrium constant.

For a water gas reaction C(s) + H_2O(g) harr CO(g) + H_2(g) at 1000^@C , the standard Gibb's energy change is -8.1 KJ mol^(-1) . Calculate the value of equilibrium constant.

For the water gas reaction C(s) + H_(2)O(g) hArr CO(g) + H_(2)(g) At 1000K , the standard Gibbs free energy change of the reaction is -8.314KJ//mol . Therefore, at 1000K the equilibrium constant of the above water gas reaction is

The standard Gibbs energy change for the reaction 2SO_2(g) +O_2(g) to 2SO_3 (g) is -142 kJ mol^(-1) at 300 K. Calculate equilibrium constant.

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) , the standard free energy is Delta G^(@)gt 0 . The equilibrium constant (K) would be