Chemistry › Redox Reactions › Balancing of redox reactions
What is the value of ' $x$ ' in order to balance the following redox reaction by ion electron method?…
What is the value of ' $x$ ' in order to balance the following redox reaction by ion electron method?
$\mathrm{x} \mathrm{H}_2 \mathrm{O}_2+\mathrm{ClO}_4 \rightarrow \mathrm{x} \mathrm{O}_2+\mathrm{ClO}_2+2 \mathrm{H}_2 \mathrm{O}$
3 4 1 2 Solution
$\mathrm{x} \mathrm{H}_2 \mathrm{O}_2+\mathrm{ClO}_4^{-} \rightarrow \mathrm{x} \mathrm{O}_2+\mathrm{ClO}_2^{-}+2 \mathrm{H}_2 \mathrm{O}$
Reduction Half Reaction
$\mathrm{ClO}_4^{-} \longrightarrow \mathrm{ClO}_2^{-}$
$4 \mathrm{e}^{-}+4 \mathrm{H}^{+}+\mathrm{ClO}_4^{-} \longrightarrow \mathrm{ClO}_2^{-}+2 \mathrm{H}_2 \mathrm{O}$
Oxidation Half Reaction,
$\begin{aligned}
& \mathrm{H}_2 \mathrm{O}_2 \longrightarrow \mathrm{O}_2 \\
& \mathrm{H}_2 \mathrm{O}_2 \longrightarrow \mathrm{O}_2+2 \mathrm{H}^{+}+2 \mathrm{e}^{-}
\end{aligned}$
Net Redox reaction
$\begin{aligned}
& {\left[4 \mathrm{e}^{-} 4 \mathrm{H}^{+}+\mathrm{ClO}_4^{-} \longrightarrow \mathrm{ClO}_2^{-}+2 \mathrm{H}_2 \mathrm{O}\right] \times 1} \\
& {\left[2 \mathrm{H}_2 \mathrm{O}_2 \longrightarrow \mathrm{O}_2+2 \mathrm{H}^{+}+2 \mathrm{e}^{-}\right] \times 2} \\
& 2 \mathrm{H}_2 \mathrm{O}_2+\mathrm{ClO}_4^{-} \longrightarrow 2 \mathrm{O}_2+\mathrm{ClO}_2^{-}+2 \mathrm{H}_2 \mathrm{O} \\
& \mathrm{x}=2
\end{aligned}$
Asked in: MHT CET 2021 (20 Sep Shift 1)
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