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Brine is electrolysed by using inert electrodes. The reaction at anode is ........

Answer»

`Cl_((aq))^(-) to 1/2 Cl_(2(g)) - e^(-) , E_(("CELL"))^(Theta) = 1.36 V`
`2H_2O_((l)) to O_(2(g)) + 4H_((aq))^(+) + 4e^(-) , E_(("cell")^(Theta) = 1.23 V`
`Na_((aq))^(+) + e^(-) to Na_((s)) , E_(("cell")"^(Theta) = 2.71 V`
`H_((aq))^(+) + e^(-) to 1/2 H_(2(g)) , E_("(cell)")^(Theta) = 0.00V`

Solution :During ELECTROLYSIS of brine, the oxidation of OXYGEN and chlorine both are possible at ANODE. However, the oxidation of oxygen requires over voltage and so chloride ions are prefrentially oxidised at anode to `Cl_2`.


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