$Mg$ (Magnesium) burns in $CO$ to produce

$KMnO_4$ acts as an oxidising agent in alkaline medium. When alkaline $KMnO_4$ is treated with $KI$,iodide ion is oxidized to

For the balanced redox reaction $xMnO_4^- + yC_2O_4^{2-} + zH^+ \to Mn^{2+} + CO_2 + H_2O$,the values of $x, y$ and $z$ are respectively:

For the ionic reaction: $XBrO_3^{-} + YCr^{+3} + ZH_2O \rightarrow pBr_2 + qHCrO_4^{-} + rH^{+}$

For the reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$. Which of the following statements is true $(T)$ or false $(F)$ regarding the nature of the reaction? The reaction is complex.

When $KMnO_4$ reacts with $Br^-$ in a basic medium to give bromate ion,the oxidation state of $Mn$ changes from $7$ to . . . . . .