Consider the change in oxidation state of Bromine corresponding to different emf values…
Chemistry · NEET · NTA Exams — Redox Reactions
Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below:
\[\begin{array}{c} \mathrm{BrO}_{4}^{-} \xrightarrow{1.82 \mathrm{~V}} \mathrm{BrO}_{3}^{-} \xrightarrow{1.5 \mathrm{~V}} \mathrm{HBrO} \\ \mathrm{Br}_{1.0652 \mathrm{~V}} \mathrm{Br}_{2} \underset{1.595 \mathrm{~V}}{\sim} \end{array}\]
Then the species undergoing disproportionation is
- Br2
- HBrO
- \(\mathrm{ErO}_{4}^{-}\)
- \(\mathrm{ErO}_{3}^{-}\)
Answer
(A) Br 2
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