Given below are two statements.Statement-I: I | vedclass

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(A) Decomposition of potassium chlorate: $2 KClO_{3(s)} \xrightarrow{\Delta} 2 KCl_{(s)} + 3 O_{2(g)}$.In $KClO_3$,the oxidation state of $Cl$ is $+5$

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Both statements-$I$ and $II$ are correct

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(A) Decomposition of potassium chlorate: $2 KClO_{3(s)} \xrightarrow{\Delta} 2 KCl_{(s)} + 3 O_{2(g)}$.In $KClO_3$,the oxidation state of $Cl$ is $+5$,and in $KCl$,it is $-1$. Since the oxidation state decreases,$Cl$ is reduced. Thus,Statement-$I$ is correct.Reaction of $Na$ with $O_2$: $4 Na_{(s)} + O_{2(g)} \rightarrow 2 Na_2O_{(s)}$.Here,$Na$ is oxidized from $0$ to $+1$ and $O$ is reduced from $0$ to $-2$. Since both oxidation and reduction occur,it is a redox reaction. Thus,Statement-$II$ is correct.

Given below are two statements.
Statement-$I$: In the decomposition of potassium chlorate,$Cl$ is reduced.
Statement-$II$: Reaction of $Na$ with $O_2$ to form $Na_2O$ is a redox reaction.
The correct answer is

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Given below are two statements.Statement-$I$: In the decomposition of potassium chlorate,$Cl$ is reduced.Statement-$II$: Reaction of $Na$ with $O_2$ to form $Na_2O$ is a redox reaction.The correct answer is