In acidic medium,potassium dichromate acts as an oxidant according to the equation,$Cr_2O_7^{2-} + 14H^{+} + 6e^- \to 2Cr^{3+} + 7H_2O$. What is the equivalent weight of $K_2Cr_2O_7$? (Molecular weight $= M$)

$6 Fe_3O_4 + 2 MnO_4^- + H_2O \to 9 Fe_2O_3 + 2 MnO_2 + 2 OH^-$ Calculate the equivalent weight of $Fe_3O_4$ in the above equation.

The equivalent weight of $K_2Cr_2O_7$ in an acidic medium is...... (Molecular weight $= M$)

Balance the following redox reactions by the ion-electron method:
$(a)$ $MnO_4^-(aq) + I^{-}(aq) \rightarrow MnO_2(s) + I_2(s)$ (in basic medium)
$(b)$ $MnO_4^-(aq) + SO_2(g) \rightarrow Mn^{2+}(aq) + HSO_4^-(aq)$ (in acidic solution)
$(c)$ $H_2O_2(aq) + Fe^{2+}(aq) \rightarrow Fe^{3+}(aq) + H_2O(l)$ (in acidic solution)
$(d)$ $Cr_2O_7^{2-} + SO_2(g) \rightarrow Cr^{3+}(aq) + SO_4^{2-}(aq)$ (in acidic solution)

From the given reaction:
$2 KMnO_4 + 3 H_2 SO_4 + 5 H_2 O_2 \longrightarrow K_2 SO_4 + 2 MnSO_4 + 8 H_2 O + 5 O_2$
Find the normality of $H_2 O_2$ solution,if $20 \ mL$ of it is required to react completely with $16 \ mL$ of $0.02 \ M \ KMnO_4$ solution.
$(Molar \ mass \ of \ KMnO_4 = 158 \ g \ mol^{-1})$

How many moles of $H_2O_2$ are required to decolorize $1 \ mol$ of $KMnO_4$ in an acidic medium (in $.5$)?