WHAT is disproportionation reaction?

Answer 1

A disproportionation reaction is one in which a species has been both oxidised and reduced (that is, the oxidation state of the related species found in the products has increased in one instance, and decreased in another, in relation to that of the species found in the reactants).

The classic example of disproportionation is the reaction between chlorine gas and dilute sodium hydroxide, although there are many others:

Cl2 + 2NaOH --> H2O + NaCl + NaClO

The oxidation state of chlorine is 0 in the reactants, but has decreased to -1 in NaCl AND has increased to +1 in sodium chlorate, NaClO.

Answer 2

In a disproportionation reaction, the same reactant is both oxidized and reduced. In other words, atoms of a substance lose electrons to a different atom of the same substance. Here's an example:

3 Cl2 + 6 OH− --> 5 Cl− + ClO3− + 3 H2O

As a reactant, chlorine has an oxidation state of 0. After the reaction, some have become Cl- with a -1 oxidation state, while others have become a part of ClO3-, in which Cl has an oxidation state of +5.

Answer 3

In these reaction, an element simultaneously undergoes oxidation as well as reduction. This is possible only when the element exhibits minimum three different oxidation states and on the reactant side, it is present in an intermediate oxidation state while higher and lower oxidation states are exhibited by it in the form of products.

Answer 4

A disproportionation reaction is a type of chemical reaction where a single substance is both oxidized and reduced simultaneously. This results in the formation of two different products with different oxidation states. An example is the decomposition of hydrogen peroxide into water and oxygen.

Answer 5

Is a reaction in which a chemical substance is oxidized and reduced at the same time.

Answer 6

It is a reaction in which the same element present in a compound undergoes oxidation as well as reduction