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3 years ago

Which type of reaction occurs in the following equation?

Chemistry

2 answers:

aniked [119]3 years ago

6 0

Answer:

The right choice is → a reduction reaction

Explanation:

From the balanced equation

3CIO⁻₍aq₎ → CIO⁻ ₍aq₎ + 2Cl⁻ ₍aq₎

we can calculate the change in oxidation number of Cl in reactant and product

in reactant ClO⁻

let x= oxidation number of Cl

and oxidation number of oxygen in its compound is (-2)

and the total charge on the ClO⁻ ion = -1

∴x + (-2) = -1 →→→ x = +1

in product Cl⁻

let x= oxidation number of Cl

and the total charge on the Cl⁻ ion = -1

∴x = -1

so the oxidation number of Cl decreases from +1 in reactant to -1 in product so it is reduction reaction.

But, disproportionation reaction is defined as the chemical reaction in which a single substance gets reduced as well as oxidized.

For a disproportionated substance , it should contain at least three oxidation states. which isn't the case here.

So, the right choice is:

→ a reduction reaction

Crazy boy [7]3 years ago

5 0

Answer:

disproportionation reaction

Explanation:

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3 years ago

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sleet_krkn [62]

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bekas [8.4K]

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