Question

4. Disproportionation reactions
Disproportionation reactions are a special type (I
of redox reactions. In a disproportionation re
reaction an element in one oxidation state is to
simultaneously oxidised and reduced. One of
the reacting substances in a w
disproportionation reaction always contains th
an element that can exist in at least three ez
oxidation states. The element in the form of n
reacting substance is in the intermediate s!
oxidation state; and both higher and lower
oxidation states of that element are formed in
the reaction. The decomposition of hydrogen
peroxide is a familiar example of the reaction,
where oxygen experiences disproportionation.
+1 - 1
+1 2 0
2H,O, (aq) → 2H,O(1) + O2(g)
(8.45)
Here the oxygen of peroxide, which is present
in-1 state, is converted to zero oxidation state
in O, and decreases to - 2 oxidation state in
HO.
Phosphorous, sulphur and chlorine
undergo disproportionation in the alkaline
medium as shown below:
3
+1
Ph(s) + 3OH (aq)+ 3H2O1) » PHÚg) + 3H2PO,
(aq)
(8.46)
+2
S (s) + 12 OH (aq) - 4s (aq) + 28,0; (aq)
+ 6H2O(1)
(8.47)
+1
-1
CL, (g) + 2 OH (aq) → CIO (aq) + C1 (aq) +
HO (1)
(8.48)​

Answer 1

Answer:

Disproportion reaction is a reaction in which a single element shows at least three oxidation state.

For Eg:

H₂O₂(aq.)=>H₂O(l)+O₂(g)

In this case, oxygen in hydrogen peroxide has oxidation number -1, while in the case of water its oxidation state is -2 and in case of oxygen molecule its oxidation state is 0. It means that oxygen shows three different oxidation states. So, this reaction is Disproportions Reaction.

Answer 2

Answer:

disproportion reactions are those in which same element in the reactant get both reduced and oxidized...

like u could see in phosphorus rxn..

0 intial ocidation state....and in reactant we observed PH3(-3) its..reduction...and H2PO2(+1)..oxidation...

so both are happening to the same element

Explanation:

hope you got it...

Good luck