Chlorine undergoes disproportionation in alkaline medium as shown below :
${aCl}_{2} (g) + {bOH}^{-} (aq) \to {cClO}^{-} (aq) + {dCl}^{-} (aq) + {eH}_{2} O (l)$
The values of $a, b, c$ and $d$ in a balanced redox reaction are respectively :

Question

Chlorine undergoes disproportionation in alkaline medium as shown below :
${aCl}_{2} (g) + {bOH}^{-} (aq) \to {cClO}^{-} (aq) + {dCl}^{-} (aq) + {eH}_{2} O (l)$

The values of $a, b, c$ and $d$ in a balanced redox reaction are respectively :

Aicharya · Accepted Answer

Chlorine undergoes disproportionation reaction in alkaline medium. It is the simultaneous oxidation-reduction. Chlorine is simultaneously reduced to chloride ion ${Cl}^{-}$ and is oxidised to ${ClO}^{-}$ ion. Halogens (e.g. Cl) have a strong tendency to accept electrons, so they act as strong oxidising agents.

The reaction is as follows,

$\Rightarrow \mathrm{Cl}_2 - 2 \mathrm{O} \mathrm{H}^- \longrightarrow \mathrm{Cl}^{-}+\mathrm{ClO}^{-}+\mathrm{H}_2 \mathrm{O}$

Hence the values of a,b,c,d are $1, 2, 1, 1 .$

Chlorine undergoes disproportionation in alkaline medium as shown below : aCl 2 ( g ) + bOH - ( aq ) → cClO…

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