In the balanced reaction $xBrO_3^- + yCr^{3+} + zH_2O \to aBr_2 + bHCrO_4^- + cH^+$,the coefficients $x, y$ and $z$ are

Number of moles of $KMnO_4$ required to oxidize one mole of $Fe(C_2O_4)$ in acidic medium is

For the redox reaction $ xMnO_{4}^{-} + yH_{2}C_{2}O_{4} + zH^{+} \rightarrow mMn^{2+} + nCO_{2} + pH_{2}O $,the values of $ x, y, m $ and $ n $ are:

The dark purple colour of $KMnO_4$ disappears in the titration with oxalic acid in acidic medium. The overall change in the oxidation number of manganese in the reaction is.

Assign $A, B, C, D$ from the given type of reaction for the following chemical equation:
$3Fe_{(s)} + 4H_2O_{(g)} \xrightarrow{\Delta} Fe_3O_{4(s)} + 4H_{2(g)}$

Write the balanced chemical equation for the following reaction in an acidic medium using the ion-electron method:
Permanganate ion $(MnO_4^-)$ reacts with sulphur dioxide gas to produce $Mn^{+2}$ and hydrogen sulphate ion $(HSO_4^-)$.