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(B) During the electrolysis of aqueous $NaCl$,the following oxidation reactions are possible at the anode:$(i)$ $Cl^{-}_{(aq)} \rightarrow \frac{1}{2}

Vedclass · Accepted Answer

$Cl^{-}_{(aq)} \rightarrow \frac{1}{2} Cl_{2_{(g)}} + e^{-}$

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(B) During the electrolysis of aqueous $NaCl$,the following oxidation reactions are possible at the anode:$(i)$ $Cl^{-}_{(aq)} \rightarrow \frac{1}{2} Cl_{2_{(g)}} + e^{-} \quad E^{o} = 1.36 \ V$$(ii)$ $2H_{2}O_{(l)} \rightarrow O_{2_{(g)}} + 4H^{+}_{(aq)} + 4e^{-} \quad E^{o} = 1.23 \ V$Although the oxidation of water has a lower standard electrode potential $(E^{o} = 1.23 \ V)$ compared to chloride ions $(E^{o} = 1.36 \ V)$,the oxidation of water requires an additional 'overpotential' to occur at a significant rate.Due to this overpotential of oxygen,the oxidation of water is kinetically hindered,and the oxidation of $Cl^{-}$ ions becomes the preferred reaction at the anode,resulting in the evolution of $Cl_{2}$ gas.

Oxidation of species depends upon its oxidation potential. An oxidation reaction is possible for the species whose $E^{o}$ value is lower. Which of the following reactions occurs at the anode during the electrolysis of aqueous $NaCl$?

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