Choose the correct option regarding the reaction $2KClO_3 \to 2KCl + 3O_2$.
$(1)$ $KClO_3$ undergoes both oxidation and reduction.
$(2)$ $Cl^{+5}$ is converted to $Cl^{-}$.
$(3)$ Oxygen in $KClO_3$ undergoes reduction.
$(4)$ This reaction cannot be called a redox reaction.

Balance the following redox reactions by the ion-electron method:
$(a)$ $MnO_{4(aq)}^- + I_{(aq)}^- \to MnO_{2(s)} + I_{2(s)}$ (in basic solution)
$(b)$ $MnO_{4(aq)}^- + SO_{2(g)} \to Mn_{(aq)}^{2+} + HSO_{4(aq)}^-$ (in acidic solution)
$(c)$ $H_2O_{2(aq)} + Fe_{(aq)}^{2+} \to Fe_{(aq)}^{3+} + H_2O_{(l)}$ (in acidic solution)
$(d)$ $Cr_2O_7^{2-} + SO_{2(g)} \to Cr_{(aq)}^{3+} + SO_{4(aq)}^{2-}$ (in acidic solution)

Which of the following reagents causes the aqueous colored solution of acidic $KMnO_4$ to become colorless?

Write the redox reaction that occurs when a zinc rod is placed in a $H_2SO_4$ solution.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$K_2Cr_2O_7 \xrightarrow{\Delta } K_2CrO_4 + Cr_2O_3 + O_2 \uparrow$

The reaction,$K_2Cr_2O_7 + m \, FeSO_4 + n \, H_2SO_4 \longrightarrow Cr_2(SO_4)_3 + p \, Fe_2(SO_4)_3 + K_2SO_4 + q \, H_2O$ when balanced,$m, n, p$ and $q$ are,respectively: