Question

Which of the following reactions are disproportionation
reactions?
(i) Cu⁺ → Cu²⁺ + Cu
(ii) 3MnO₄⁻ + 4H⁺ → 2MnO₄⁻ +MnO₂ + 2H₂O
(iii) 2KMnO₄ → K₂MnO₄ + MnO₂ + O₂
(iv) 2MnO₄⁻ + 3Mn²⁺ + 2H₂O → 5MnO₂ + 4H⁺
(a) (i) (b) (i), (ii) and (iii)
(c) (ii), (iii) and (iv) (d) (i) and (iv)

Answer 1

Which of the following reactions are disproportionation

reactions?

(i) Cu⁺ → Cu²⁺ + Cu

(ii) 3MnO₄⁻ + 4H⁺ → 2MnO₄⁻ +MnO₂ + 2H₂O

(iii) 2KMnO₄ → K₂MnO₄ + MnO₂ + O₂

(iv) 2MnO₄⁻ + 3Mn²⁺ + 2H₂O → 5MnO₂ + 4H⁺

(a) (i) (b) (i), (ii) and (iii)

(c) (ii), (iii) and (iv)

(d) (i) and (iv)

Answer 2

1,and 2 are the disproportionation reaction.

Explanation:

• Disproportionation reaction is defined as those reaction where a particular element is both oxidised and reduced simultaneously in a reaction.

• Here in the 1st reaction, we can see that copper in the form of cuprous ions are undergoing subsequent oxidation to cupric form as well as getting reduced to form metallic copper.

• So the +1 oxidation state of cuprous is getting oxidised to +2 state of cupric and 0 state of metallic copper.

• In the second case, the Manganate ion is getting oxidised to permanganate ion and also getting reduced to the manganese dioxide too.

• So the +6 oxidation state of the manganate ion is getting oxidised to +7 of the permanganate ion, as well as reduced to +4 state of the manganese dioxide ion.

• The reaction of number 3 is not a disproportionation reaction as both the products are reduced form of manganese.

• The last reaction is a comproportionation reaction.

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