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:

YESPYQ · Accepted Answer

Correct answer: a) 1, 2, 1 and 1. Balanced redox equation in alkaline medium: Cl₂ + 2OH⁻ → ClO⁻ + Cl⁻ + H₂O To balance: Unbalanced form given in question: aCl₂ + bOH⁻ → cClO⁻ + dCl⁻ + eH₂O Balanced form: a = 1, b = 2, c = 1, d = 1, e = 1 Hence, the correct option is: A (1, 2, 1, 1).

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

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