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 :

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

Quantrex Academy · Accepted Answer

Correct answer: A. 1, 2, 1and1

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.

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

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...

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