In order to oxidize a mixture of $1 \text{ mole}$ each of $FeC_2O_4$, $Fe_2(C_2O_4)_3$, $FeSO_4$, and $Fe_2(SO_4)_3$ in an acidic medium, the number of moles of $KMnO_4$ required is:

Number of moles of $MnO_4^{-}$ required to oxidise one mole of ferrous oxalate completely in acidic medium will be $:-$ (in $mole$)

$I^{-}(aq.) + MnO_4^{-}(aq.) \xrightarrow{H^{+}} X + Mn^{2+}(aq.)$
$I^{-}(aq.) + MnO_4^{-}(aq.) \xrightarrow{\text{Neutral or weakly } OH^{-}} Y + MnO_2$
$MnO_4^{-}(aq.) + Mn^{2+}(aq.) \xrightarrow{ZnSO_4} Z + 4H^{+}$
Products $X, Y$ and $Z$ are respectively :

Chlorine oxidises sulphur dioxide in the presence of water to give an oxyacid $A$. Chlorine also oxidises iodine in the presence of water to give an oxyacid $B$. The oxidation states of $S$ and $I$ in $A$ and $B$ are respectively

Consider the reactions:
$2S_2O_3^{2-}(aq) + I_2(s) \to S_4O_6^{2-}(aq) + 2I^-(aq)$
$S_2O_3^{2-}(aq) + 2Br_2(l) + 5H_2O(l) \to 2SO_4^{2-}(aq) + 4Br^-(aq) + 10H^+(aq)$
Why does the same reductant,thiosulphate,react differently with iodine and bromine?

Among $C$,$S$,and $P$,the element$(s)$ that produce$(s)$ $SO_{2}$ on reaction with hot conc. $H_{2}SO_{4}$ is / are