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Types of Redox Reactions

Which of the ...

Question

Which of the following is/are disproportionation reactions?

2 O_{3} ⟶ 3 O_{2}

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4 K C l O_{3} ⟶ 3 K C l O_{4} + K C l

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2 H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}

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2 K O_{2} + 2 H_{2} O ⟶ 4 K O H + 3 O_{2}

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Solution

The correct options are
A $2 O_{3} ⟶ 3 O_{2}$
B $4 K C l O_{3} ⟶ 3 K C l O_{4} + K C l$
C $2 H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}$
D $2 K O_{2} + 2 H_{2} O ⟶ 4 K O H + 3 O_{2}$
The various redox reactions are given below:
$2 O_{3} ⟶ 3 O_{2}$
+2/-2 0
$4 K C l O_{3} ⟶ 3 K C l O_{4} + K C l$
+5 +7 -1
$2 H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}$
-1 -2 0
$2 K O_{2} + 2 H_{2} O ⟶ 4 K O H + 3 O_{2}$
-1/2 -2 0
Thus, we can see that all the above reactions are disproportionation reactions.

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N a_{2} O + C O_{2} \to (Z - -)

2 C u^{+}

\to

C u^{2 +}

C u^{0}

3 M n O_{4}^{2 -}

4 H^{+}

\to

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2 K M n O_{4}

△ - \to

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O_{2}

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⟶

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2 M n O_{2} + 4 K O H + O_{2} ⟶ {2 K}_{2} M n O_{4} + 2 H_{2} O

2 O_{3} ⇌ 3 O_{2}

O_{3} ⇌ O_{2} + O

O + O_{2} \to 2 O_{2}

2 O_{3} \to 3 O_{2}

O_{3} ⇌ O_{2} + O . . . . . (f a s t)

O + O_{2} \to 2 O_{2} . . . . . (s l o w)

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