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(D) In the reaction $2KClO_3 	o 2KCl + 3O_2$:$1$. The oxidation state of $Cl$ in $KClO_3$ is $+5$ and in $KCl$ is $-1$. Since the oxidation state dec

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$TTFF$

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(D) In the reaction $2KClO_3 	o 2KCl + 3O_2$:$1$. The oxidation state of $Cl$ in $KClO_3$ is $+5$ and in $KCl$ is $-1$. Since the oxidation state decreases,$Cl$ undergoes reduction. Thus,statement $(2)$ is True.$2$. The oxidation state of $O$ in $KClO_3$ is $-2$ and in $O_2$ is $0$. Since the oxidation state increases,$O$ undergoes oxidation. Thus,statement $(3)$ is False.$3$. Since both oxidation and reduction occur in the same reaction,it is a redox reaction. Thus,statement $(4)$ is False.$4$. Since $KClO_3$ contains both the element being oxidized $(O)$ and the element being reduced $(Cl)$,it undergoes both oxidation and reduction. Thus,statement $(1)$ is True.Therefore,the sequence of truth values is $(1)=T, (2)=T, (3)=F, (4)=F$,which corresponds to $TTFF$.

Choose the correct option regarding the reaction $2KClO_3 \to 2KCl + 3O_2$.
$(1)$ $KClO_3$ undergoes both oxidation and reduction.
$(2)$ $Cl^{+5}$ is converted to $Cl^{-}$.
$(3)$ Oxygen in $KClO_3$ undergoes reduction.
$(4)$ This reaction cannot be called a redox reaction.

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Choose the correct option regarding the reaction $2KClO_3 \to 2KCl + 3O_2$.$(1)$ $KClO_3$ undergoes both oxidation and reduction.$(2)$ $Cl^{+5}$ is converted to $Cl^{-}$.$(3)$ Oxygen in $KClO_3$ undergoes reduction.$(4)$ This reaction cannot be called a redox reaction.