The standard change in Gibbs energy for the reaction: `H_2O hArr H^+ +OH^-` at `25^@C` is :

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.

Calculate the standard reduction potential for the reaction H_2O+ e to 1/2 H_2+OH^- using the Nernst equation and the fact that the standard reduction potential for the reaction H^+ + e to 1/2 H_2 is by definition equal to 0.00V at 25^@C

The standard reduction potential of the reaction H_(2)O+e^(-) rarr 1/2 H_(2) +OH , at 298 K, is

The standard reduction potential of the reaction, 2H_(2)O+2e rarr H_(2)+2OH^(-) is -0.8277V at 25^(@)C . Find the value of the equilibrium constant of the reaction 2H_(2)Orarr H_(3)O^(+)+OH^(-) at the same temperature.