JEE MAIN - Chemistry (2024 - 29th January Morning Shift - No. 7)
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
Explanation
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$$$\Rightarrow \mathrm{Cl}_2+2 \overline{\mathrm{O}} \mathrm{H} \longrightarrow \mathrm{Cl}^{-}+\mathrm{ClO}^{-}+\mathrm{H}_2 \mathrm{O}$$$
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