Question

Which type of reaction occurs in the following equation?

3CIO (aq) →→ CIO, (aq) + 2Cl(aq)
an oxidation reaction
a reduction reaction
a synthesis reaction
a disproportionation reaction

Answer 1

disproportionation reaction

Step-by-step explanation:

Answer 2

The right choice is → a reduction reaction

Step-by-step 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