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Given 2H(2)O rarr O2 + 4H^+ + 4e^- , E0 ...

Given `2H_(2)O rarr O_2 + 4H^+ + 4e^-` , `E_0 = -1.23 V`. Calculate electrode potential at pH = 5.

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Given that, Co^(3+) +e^(-)rarr Co^(2+) , E^(@) = +1.82 V 2H_(2)O rarr O_(2) +4H^(+) +4e^(-), E^(@) =- 1.23 V . Explain why Co^(3+) is not stable in aqueous solutions.

Given that, Co^(3+) +e^(-)rarr Co^(2+) E^(@) = +1.82 V 2H_(2)O rarr O_(2) +4H^(+) +4e^(-), E^(@) =- 1.23 V . Explain why Co^(3+) is not stable in aqueous solutions.

Given that, Co^(3+) +e^(-)rarr Co^(2+) E^(@) = +1.82 V 2H_(2)O rarr O_(2) +4H^(+) +4e^(-), E^(@) =- 1.23 V . Explain why Co^(3+) is not stable in aqueous solutions.

The reaction 2H_2O (l) rarr 4H^+ +O2+2e^-

Calculate equilibrium constant for the reaction 2H_2O rarr H_3O^(oplus) + OH^- Given H_2O + 2e rarr H_2 + 2OH^- Standard reduction potentials is -0.83 V at 25^@C .

For the half cell, +2H^(+)2e^(-).E^(0)= 1.30 V. At pH = 2 , electrode potential of the given quinhydrone half cell is :

The electrode potential of some half cell reactions are : Cl_(2) + 2e^(-) rarr 2 Cl^(-)(aq), E^(@) = + 1.36 V O_(2)+2H^(+)(aq) + 2e^(-) rarr H_(2)O_(2) (aq) , E^(@) = + 0.65 V F_(2)+2e^(-) rarr 2F^(-)(aq), E^(@) = + 2.87 V H_(2)O+ 2e^(-) rarr H_(2)(g) + 2OH^(-) (aq), E^(@) = - 0.83 V The strongest oxidising agent is :