$MnO_4^-$ on reduction in acidic medium forms

When thiosulphate ion is oxidised by iodine,which one of the following ions is produced?

$Na_2S_2O_3$ reacts with moist $Cl_2$ to form $Na_2SO_4$, $HCl$, and $X$. Which one of the following is $X$?

$A$ solution of $Na_2S_2O_3$ is standardized iodometrically against $0.167 \ g$ of $KBrO_3$ where $BrO_3^-$ changes to $Br^-$. This process requires $45 \ mL$ of the $Na_2S_2O_3$ solution. What is the strength of the $Na_2S_2O_3$ in $N$?
$[Mw \text{ of } KBrO_3 = 167]$

Permanganate $(VII)$ ion,$MnO_4^-$,in basic solution oxidises iodide ion,$I^-$,to produce molecular iodine $(I_2)$ and manganese $(IV)$ oxide $(MnO_2)$. Write a balanced ionic equation to represent this redox reaction.

Which of the following is a redox reaction?