Which one of the following reactions is a redox reaction?

C u S O_{4} + 4 N H_{3} \to [C u (N H_{3})_{4}] S O_{4}

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N a_{2} S O_{4} + B a C l_{2} \to B a S O_{4} + 2 N a C l

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

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2 C u S O_{4} + 4 K I \to C u_{2} I_{2} + 2 K_{2} S O_{4} + I_{2}

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Solution

The correct option is D $2 C u S O_{4} + 4 K I \to C u_{2} I_{2} + 2 K_{2} S O_{4} + I_{2}$
The reaction in which change in oxidation numbers of some of the atoms takes place is termed as a redox reaction.
$(a) + 2 + 6 - 2 C u S O_{4} + - 3 + 1 4 N H_{3} \to + 2 - 3 - 1 + 6 - 2 [C u (N H_{3})_{4}] S O_{4}$
No change in oxidation number of any of the atoms.
$(b) + 1 + 6 - 2 N a_{2} S O_{4} + + 2 - 1 B a C l_{2} \to + 2 + 6 - 2 B a S O_{4} + + 1 - 1 2 N a C l$
No Change in oxidation number of any of the atoms.
$(c) + 4 - 2 S O_{2} + + 1 - 2 H_{2} O \to + 1 + 4 - 2 H_{2} S O_{3}$
No change in oxidation number of any of the atoms.
$(d) + 2 + 6 - 2 2 C u S O_{4} + + 1 - 1 4 K I \to + 1 - 1 C u_{2} I_{2} + + 1 + 6 - 2 2 K_{2} S O_{4} +_{2}$
Oxidation number of $C u$ decreases from $+ 2 t o + 1$ and oxidation number of iodine increases from $- 1 t o 0$ .
Thus, out of the above four reactions, the reaction (d) is a redox reaction.

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Similar questions

C u S O_{4} + 4 N H_{3} \to C u (N H_{3})_{4}] S O_{4}

N a_{2} S O_{4} + B a C l_{2} \to B a S O_{4} + 2 N a C l

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

2 C u S O_{4} + 4 K I \to C u_{2} I_{2} + 2 K_{2} S O_{4} + I_{2}

2 C u S O_{4} + 4 K I \to C u_{2} I_{2} + 2 K_{2} S O_{4} + I_{2}

C u S O_{4}

(M w = 159.5 g

m o l^{- 1})

2 C u S O_{4} + 4 K I ⟶ C u_{2} I_{2} + 2 K_{2} S O_{4} + I_{2}

C u S O_{4}

B a S O_{4}

[C u (N H_{3})_{4}] S O_{4}

B a C l_{2}

H {N O}_{3} + C a {(O H)}_{2} \to C a {({N O}_{3})}_{2} + H_{2} O

N a C l + A g {N O}_{3} \to A g C l + N a {N O}_{3}

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

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