Chlorine undergoes disproportionation in alkaline medium as shown below:

\({\mathrm{aCl}}_{2}(\mathrm{g})+{\mathrm{bOH}}^{−}(\mathrm{aq})\to {\mathrm{cClO}}^{−}(\mathrm{aq})+{\mathrm{dCl}}^{−}(\mathrm{aq})+{\mathrm{eH}}_{2}\mathrm{O}(\mathrm{l})\)

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:

\({\mathrm{aCl}}_{2}(\mathrm{g})+{\mathrm{bOH}}^{−}(\mathrm{aq})\to {\mathrm{cClO}}^{−}(\mathrm{aq})+{\mathrm{dCl}}^{−}(\mathrm{aq})+{\mathrm{eH}}_{2}\mathrm{O}(\mathrm{l})\)

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

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Chlorine undergoes disproportionation in alkaline medium as shown below: \({\mathrm{aCl}}_{2}(\mathrm{g})+{\mathrm{bOH}}…

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