How many electrons are lost in the following transformation?
$3Fe + 4H_2O \to Fe_3O_4 + 4H_2$

In the following balanced reaction,
$X\,MnO_4^- + Y\,C_2O_4^{2-} + Z\,H^+ \rightleftharpoons X\,Mn^{2+} + 2Y\,CO_2 + \frac{Z}{2}\,H_2O$
values of $X, Y$ and $Z$ respectively are

Consider the following equations:
$2 Fe^{2+} + H_2O_2 \rightarrow x A + y B$
(in basic medium)
$2 MnO_4^{-} + 6 H^{+} + 5 H_2O_2 \rightarrow x' C + y' D + z' E$
(in acidic medium)
The sum of the stoichiometric coefficients $x, y, x', y'$ and $z'$ for products $A, B, C, D$ and $E,$ respectively,is............

$C +$ Conc. $H_2SO_4 \xrightarrow{\Delta} X + Y + H_2O$. $X$ and $Y$ in the above reaction are:

In the given reaction,calculate the number of electrons lost by iron:
$3Fe + 4H_2O \to Fe_3O_4 + 4H_2$

The oxidation state of chromium in the final product formed by the reaction between $KI$ and acidified potassium dichromate solution is