Chlorine undergoes disproportionation in alkaline medium as shown below : $\mathrm{aCl}_{2(\mathrm{~g})}+\mathrm{b} \mathrm{OH}_{(\mathrm{aq})}^{-} \rightarrow \mathrm{c} \mathrm{ClO}_{(\mathrm{aq)}}^{-}+\mathrm{d} \mathrm{Cl}_{(\mathrm{aq})}^{-}+\mathrm{e} \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$ 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 :

$\mathrm{aCl}_{2(\mathrm{~g})}+\mathrm{b} \mathrm{OH}_{(\mathrm{aq})}^{-} \rightarrow \mathrm{c} \mathrm{ClO}_{(\mathrm{aq)}}^{-}+\mathrm{d} \mathrm{Cl}_{(\mathrm{aq})}^{-}+\mathrm{e} \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$

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

3, 4, 4 and 2

1, 2, 1 and 1

2, 4, 1 and 3

2, 2, 1 and 3

Solution

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