Not an example of redox reaction

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$2 B a O + O_{2} \to 2 B a O_{2}$

$B a O_{2} + H_{2} S O_{4} \to B a S O_{4} + H_{2} O_{2}$

$2 K C l O_{3} \to 2 K C l + 3 O_{2}$

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

answer is B.

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Detailed Solution

In option (A) the oxidation state of oxygen in $BaO$ and $O_{2}$ are $- 2$ and $0$ , the oxidation state of oxygen in ${BaO}_{2}$ is $- 1$ . There involves redox reaction
In option (B) the oxidation state of oxygen in ${BaO}_{2}$ and $H_{2} O_{2}$ is $- 1$ , the oxidation state of sulfur in $H_{2} {SO}_{4}$ and $B a S O_{4}$ is $+ 6$ . There is no change in oxidation states of atoms in reactants and products
In option (C) the oxidation state of chlorine in ${KClO}_{3}$ and $KCl$ are $+ 5$ and $- 1$ . There involves redox reaction
In option (D) the oxidation state of sulfur in ${SO}_{2}$ and $H_{2} S$ is $+ 4$ and $- 2$ respectively, whereas in the product elemental sulfur the oxidation state is $0$ . There involves redox reaction