`E_"cell"^@` for the reaction , `2H_2O to H_3O^(+) + OH^(-)` at `25^@C` is -0.8277 V. The equilibrium constant for the reaction is

The standard reduction potential at 25^@C of the reaction 2H_2O+2e^(-) leftrightarrow H_2 +2OH^(-) is -0.8277 volt. Calculate the equilibrium constant for the reaction 2H_2O=H_3O^+ +OH^(-) at 25^@C

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.

The standard reduction potential at 25^(@)C of the reaction 2H_(2)O+2e^(-)hArrH_(2)+2overset(Θ)(O)H is -0.8277V . Calculate the equilibrium constant for the reaction. 2H_(2)OhArrH_(3)O^(o+)+overset(Θ)(O)H at 25^(@)C .

The standard reduction potential at 25^(@)C of the reaction 2H_(2)O+2e^(-)hArrH_(2)+2overset(Θ)(O)H is -0.8277V . Calculate the equilibrium constant for the reaction. 2H_(2)OhArrH_(3)O^(o+)+overset(Θ)(O)H at 25^(@)C .

The E_("cell") of the reaction MnO_(4)^(-)+Fe^(+2)+H^(+)rarrMn^(+)+H_(2)O is 0.59 V at 25^(@)C The equilibrium constant for the reaction is

The E_("cell") of the reaction MnO_(4)^(-)+Fe^(+2)+H^(+)rarrMn^(2+)+H_(2)O is 0.59 V at 25^(@)C The equilibrium constant for the reaction is