Chlorine undergoes disproportionation in alkaline medium as shown below: aCl 2(~g) +b OH (aq) ⁻ → c ClO (aq) ⁻+d Cl (aq) ⁻+e H₂ O (l) The values of a, b, c and d in a balanced redox reaction are respectively:

Redox Reactions and Electrochemistry: JEE Main 2024 Chemistry question

JEE Main 2024 · 29 Jan, Morning shift · Q1789

JEE Main 202429 Jan, Morning shiftChemistryMediumRedox Reactions and Electrochemistry138× since 2002

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 :

JEE Main 2024 · 29 Jan, Morning shift · Q1789

JEE Main 202429 Jan, Morning shiftChemistryMediumRedox Reactions and Electrochemistry138× since 2002

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 :