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(C) First,assign oxidation numbers to the elements in the reaction: $I_2^0 + K^{+1}Cl^{+5}O_3^{-2} \rightarrow I^{+1}Cl^{-1} + K^{+1}I^{+5}O_3^{-2}$.I

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Oxidation number of $Cl$ decreases by $6$

Vedclass · Answer

(C) First,assign oxidation numbers to the elements in the reaction: $I_2^0 + K^{+1}Cl^{+5}O_3^{-2} \rightarrow I^{+1}Cl^{-1} + K^{+1}I^{+5}O_3^{-2}$.In this reaction,$I_2$ (oxidation number $0$) is oxidized to $I^{+1}$ (in $ICl$) and $I^{+5}$ (in $KIO_3$).Since $I_2$ is being oxidized,it acts as a reducing agent.$Cl$ in $KClO_3$ changes from $+5$ to $-1$ (in $ICl$).The change in oxidation number of $Cl$ is $|-1 - 5| = 6$. Thus,the oxidation number of $Cl$ decreases by $6$.Therefore,the statement 'Oxidation number of $Cl$ decreases by $6$' is correct.

Identify the correct statement for the reaction: $I_2 + KClO_3 \xrightarrow{\Delta} ICl + KIO_3$

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