$2MnO_4^{-} + 5H_2O_2 + 6H^{+} \to 2Z + 5O_2 + 8H_2O$. In this reaction $Z$ is

Number of moles of $KMnO_{4}$ reduced by $1 \ mol$ of $I^{-}$ in basic medium is

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.

Permanganate ion reacts with bromide ion in basic medium to give manganese dioxide and bromate ion. Write the balanced ionic equation for the reaction.

For a redox reaction,how many moles of electrons will one mole of $MnO_4^-$ accept in an acidic medium?

In neutral or faintly alkaline solution,$8$ moles of permanganate anion quantitatively oxidize thiosulphate anions to produce $X$ moles of a sulphur containing product. The magnitude of $X$ is