Which of the following is an intermolecular redox reaction?

2 O C H - C H O ⊖ O H - ----- \to H O C H_{2} - C H_{2} O H

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2 C_{6} H_{5} C H O A l {(O C_{2} H_{5})}_{3} - ------ \to C_{6} H_{5} C O O H + C_{6} H_{5} C H_{2} O H

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4 C r O_{5} + 6 H_{2} S O_{4} ⟶ 2 {C r}_{2} {(S O_{4})}_{3} + 6 H_{2} O + 7 O_{2}

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{A s}_{2} S_{3} + H N O_{3} ⟶ H_{3} A s O_{4} + H_{2} S O_{4} + N O

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Solution

The correct option is D ${A s}_{2} S_{3} + H N O_{3} ⟶ H_{3} A s O_{4} + H_{2} S O_{4} + N O$
Option D: It has redox reaction:
$A s_{2} S_{3} + H N O_{3} \to H_{3} A s O_{4} + H_{2} S O_{4} + N O$
As in this reaction the Oxidation state (O.S.) of S in $A s_{2} S_{3}$ is -2, whereas in $H_{2} S O_{4}$ it is +6, means it is oxidised.
In the same way, O.S. of N in $H N O_{3}$ is +5 whereas in NO it is +2, means it is reduced. So as one is reducing and other is oxidising hence this is intermolecular redox reaction.
In other options it does not occur.

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Similar questions

4 C r O_{5} + 6 H_{2} S O_{4} \to 2 C r_{2} (S O_{4})_{3} + 6 H_{2} O + 7 O_{2}

4 C r O_{5} + 6 H_{2} S O_{4} \to 2 C r_{2} (S O_{4})_{3} + 6 H_{2} O + 7 O_{2}

{3 C H}_{3} {C H}_{2} O H + 2 K_{2} {C r}_{2} O_{7} + 8 H_{2} S O_{4} ⟶ 3 {C H}_{3} C O O H + 2 {C r}_{2} {(S O_{4})}_{3}

+ {2 K}_{2} S O_{4} + 11 H_{2} O

{C H}_{3} {C H}_{2} O H

2 C_{6} H_{5} C H O + {O H}^{-} ⟶ C_{6} H_{5} C O O^{-} + C_{6} H_{5} {C H}_{2} O H

A s_{2} S_{3} + H N O_{3} \to H_{3} A s O_{4} + H_{2} S O_{4} + N O

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