$H_2O_2$ reduces $MnO_4^-$ ion to:

Balance the redox reaction where $Fe^{+2}$ in an acidic medium reduces $Cr_2O_7^{-2}$ ion to $Cr^{+3}$ ion,while $Fe^{+2}$ itself is oxidized to $Fe^{+3}$.

What is the oxidation state of chromium in the final product formed by the reaction between $KI$ and acidic $K_2Cr_2O_7$ solution?

The heating of $(NH_4)_2Cr_2O_7$ produces another chromium compound along with $N_2$ gas. The change of the oxidation state of $Cr$ in the reaction is

Consider the following reaction:
$xMnO_4^{-} + yC_2O_4^{2-} + zH^{+} \rightarrow xMn^{2+} + 2yCO_2 + \frac{z}{2}H_2O$
The values of $x, y$ and $z$ in the reaction are,respectively:

Find the equivalent weight of $MnO_4^{-}$ for acid medium reactions. (Atomic weight of $Mn = 55$,Atomic weight of $O = 16$)