What is a disproportionation reaction? Use the following...

What is a disproportionation reaction? Use the following reduction potentials $\mathrm{ClO}_{3}^{-}+3 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{HClO}_{2}+\mathrm{H}_{2} \mathrm{O} \quad \mathscr{8}^{*}=1.21 \mathrm{~V}$ $\mathrm{HClO}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{HClO}+\mathrm{H}_{2} \mathrm{O} \quad \mathscr{8}^{*}=1.65 \mathrm{~V}$ to predict whether $\mathrm{HClO}_{2}$ will disproportionate.

What is a disproportionation reaction? Use the following reduction potentials
$\mathrm{ClO}_{3}^{-}+3 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{HClO}_{2}+\mathrm{H}_{2} \mathrm{O} \quad \mathscr{8}^{*}=1.21 \mathrm{~V}$
$\mathrm{HClO}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{HClO}+\mathrm{H}_{2} \mathrm{O} \quad \mathscr{8}^{*}=1.65 \mathrm{~V}$
to predict whether $\mathrm{HClO}_{2}$ will disproportionate.

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Key Concepts

Electrochemical Prediction of Reaction Spontaneity

By comparing the standard reduction potentials for different half-reactions, one can predict whether a reaction is spontaneous. In the context of disproportionation, if the potential for the oxidation process and the potential for the reduction process multiply in such a way that the overall reaction is thermodynamically favorable, the species may disproportionate.

Standard Reduction Potential

Standard reduction potentials quantify the tendency of a species to gain electrons (be reduced) under standard conditions. These values are critical for analyzing redox reactions because they help predict the direction of electron flow and the feasibility of redox processes.

Disproportionation Reaction

A disproportionation reaction is a redox process where a single chemical species undergoes simultaneous oxidation and reduction to form two different products that contain the element in two distinct oxidation states. This internal redox change results in one part of the species being reduced while another is oxidized.

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