In the electrolysis of aqueous sodium chlorid | vedclass

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(D) In an aqueous solution of sodium chloride,the following ions are present: $Na^{+}$,$Cl^{-}$,$H^{+}$,and $OH^{-}$.At the anode,oxidation occurs. Th

Vedclass · Accepted Answer

$Cl^{-}_{(aq)} \rightarrow \frac{1}{2}Cl_{2(g)} + e^{-} ; E^{\circ} = 1.36 \ V$

Vedclass · Answer

(D) In an aqueous solution of sodium chloride,the following ions are present: $Na^{+}$,$Cl^{-}$,$H^{+}$,and $OH^{-}$.At the anode,oxidation occurs. The two possible oxidation reactions are:$1$) $2H_{2}O_{(l)} \rightarrow O_{2(g)} + 4H^{+}_{(aq)} + 4e^{-} ; E^{\circ} = 1.23 \ V$$2$) $Cl^{-}_{(aq)} \rightarrow \frac{1}{2}Cl_{2(g)} + e^{-} ; E^{\circ} = 1.36 \ V$Although the standard electrode potential for water oxidation is lower,the oxidation of $Cl^{-}$ is kinetically preferred due to the overpotential of oxygen evolution on the electrode surface. Thus,$Cl^{-}$ ions are preferentially oxidized at the anode.

In the electrolysis of aqueous sodium chloride solution,which of the half-cell reaction will occur at the anode?

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