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Types of Redox Reactions

Identify disp...

Question

Identify disproportionation reaction.

A

C H_{3} + 2 O_{2} \to C O_{2} + 2 H_{2} O

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B

C H_{4} + 4 C l_{2} \to C C l_{4} + 4 H C l

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C

2 F_{2} + 2 O H^{-} \to 2 F^{-} + O F_{2} + H_{2} O

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D

2 N O_{2} + 2 O H^{-} \to N O_{2}^{-} + N O_{3}^{-} + H_{2} O

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Solution

The correct option is C $2 N O_{2} + 2 O H^{-} \to N O_{2}^{-} + N O_{3}^{-} + H_{2} O$
In the reaction, the same element, i.e., $N$ is reduced as well as oxidised, so it is a disproportionation reaction.

Hence, option $D$ is correct.

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Similar questions

Q. Match the column I with column II to identify the products of oxidation of alkanes and mark the appropriate choice.

	Column I		Column II
(A)	$C H_{4} + 2 O_{2} K M n O_{4} - ---- \to [O]$	(i)	$H C O O H + H_{2} O$
(B)	$2 C H_{4} + O_{2} C u / 523 K - ----- \to 100 a t m$	(ii)	$C O_{2} + 2 H_{2} O$
(C)	$C H_{4} + O_{2} M o_{2} O_{3} - ----- \to Δ$	(iii)	$2 C H_{3} O H$
(D)	$C H_{4} + \frac{3}{2} O_{2} (C H_{3} C O O)_{2} M n - --------- \to$	(iv)	$H C H O + H_{2} O$

Q. Standard heats of formation for

C {C l}_{4}, H_{2} O, {C O}_{2}

H C l

298 K

- 25.5, - 57.8, - 94.1

- 22.1 k J / m o l

respectively.
For the reaction, what will be

Δ H

?

C {C l}_{4} + 2 H_{2} O \to {C O}_{2} + 4 H C l

Q. What is the equivalent weight of

O_{2}

in the following reaction?

H_{2} O + \frac{1}{2} O_{2} + 2 e^{-} ⟶ 2 O H^{-}

Q. Balance the following chemical equation in basic medium:

M n O_{4}^{-} (a q) + B r^{-} (a q) \to M n O_{2} (s) + B r O_{3}^{-} (a q)

C r_{2} O_{7}^{_{2}} + H_{2} O + 3 S O_{2} \to 2 C r^{+ 3} + 2 O H^{-} + 3 S O_{4}^{- 2}

write down to oxidation and reduction reaction

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