Question

Which of the following is not an example of disproportionation reaction?
a) Cl2 + 2NaOH → NaCl + NaOCl + H2O
b) PA+ 3NaOH + 3H20 = PH+ 3NaH,PO
c) 2NaOH + 2F, → 2NaF + OF2 + H2O
d) 2H2O2 → 2H2O + O2​

Answer 1

Explanation:

Disproportionation reaction is that reaction in which same substance undergoes oxidation as well as reduction to give two different products.

In A) reaction,oxidation state of chlorine changes from -1 in HCl to 0 in Cl

2

and -1 in MnCl

2

.Here chlorine undergoes only oxidation.So this is not disproportionation.

In B) reaction,oxidation state of oxygen changes from -1 in H

2

O

2

to 0 in O

2

and -2 in H

2

O.Here oxygen undergoes only oxidation as well as reduction.So this is disproportionation reaction.

In C) reaction,oxidation state of chlorine changes from +5 in KClO

3

to -1 in KCl and +7 in KClO

4

.Here chlorine undergoes only oxidation as well as reduction.So this is disproportionation reaction.

In D) reaction,oxidation state of chlorine changes from 0 in Cl

2

to -1 in NaCl and +5 in NaClO

3

.Here chlorine undergoes only oxidation as well as reduction.So this is disproportionation reaction.

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