In the neutral or faintly alkaline medium,$KMnO_4$ oxidises iodide into iodate. The change in oxidation state of manganese in this reaction is from?

$Cr _2 O _7^{2-} \rightarrow Cr ^{3+}_{aq}$
How many moles of $Sn^{2+}$ will be oxidized by $1 \ mol \ Cr_2O_7^{2-}$ into $Sn^{4+}$?

Consider the following redox reaction taking place in acidic medium: $BH_{4}^{-}(aq) + ClO_{3}^{-}(aq) \rightarrow H_{2}BO_{3}^{-}(aq) + Cl^{-}(aq)$. If the Nernst equation for the above balanced reaction is $E_{cell} = E_{cell}^{o} - \frac{RT}{nF} \ln Q$,then the value of $n$ is . . . . . . . (Nearest integer)

$aIO_3^- + bI^- + 6H^+ \to cI_2 + 3H_2O$
In the above reaction,the coefficients $a$,$b$,and $c$ are respectively:

Number of moles of $MnO_4^-$ required to oxidize one mole of ferrous oxalate completely in acidic medium will be .......... $moles$.

Write the balanced chemical equation for the following reaction:
$Cl_2O_7$ in the gaseous state combines with an aqueous solution of hydrogen peroxide $(H_2O_2)$ in an acidic medium to give chlorite ion $(ClO_2^-)$ and oxygen gas $(O_2)$. (Balance by the ion-electron method)