KI is oxidised into I_2 by using the reagent | vedclass

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(D) $KI$ can be oxidized to $I_2$ by various oxidizing agents:$1$. $KMnO_4$ in neutral or slightly alkaline medium: $2 KMnO_4 + KI + H_2O \rightarrow

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All of these

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(D) $KI$ can be oxidized to $I_2$ by various oxidizing agents:$1$. $KMnO_4$ in neutral or slightly alkaline medium: $2 KMnO_4 + KI + H_2O \rightarrow 2 MnO_2 + 2 KOH + KIO_3$ (Note: $KI$ is oxidized to $I_2$ or $IO_3^-$ depending on conditions).$2$. Ozone $(O_3)$ in alkaline solution: $2 KI + O_3 + H_2O \rightarrow I_2 + 2 KOH + O_2$.$3$. $CuSO_4$ solution: $2 CuSO_4 + 4 KI \rightarrow Cu_2I_2 + 2 K_2SO_4 + I_2$.Since all the given reagents can oxidize $KI$ to $I_2$,the correct option is $D$.

List-$I$ (Reaction)	List-$II$ (Type of redox reaction)
$A$. $N_{2(g)} + O_{2(g)} \rightarrow 2 NO_{(g)}$	$I$. Decomposition
$B$. $2 Pb(NO_3)_{2(s)} \rightarrow 2 PbO_{(s)} + 4 NO_{2(g)} + O_{2(g)}$	$II$. Displacement
$C$. $2 Na_{(s)} + 2 H_2 O_{(l)} \rightarrow 2 NaOH_{(aq)} + H_{2(g)}$	$III$. Disproportionation
$D$. $2 NO_{2(g)} + 2 OH^-_{(aq)} \rightarrow NO^-_{2(aq)} + NO^-_{3(aq)} + H_2 O_{(l)}$	$IV$. Combination

$KI$ is oxidised into $I_2$ by using the reagent

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