Identify the type of reaction for the following: ${P_4} + NaOH + {H_2}O \to Na{H_2}P{O_2} + P{H_3}$

The $Mn^{3+}$ ion is unstable in solution and undergoes disproportionation to give $Mn^{2+}$,$MnO_2$,and $H^{+}$ ion. Write a balanced ionic equation for the reaction.

In the following reaction,assign the state for the underlined atom in the product of complete hydrolysis at $R.T.$:
$\underline{Cl}O_2 + H_2O \longrightarrow HClO_2 + HClO_3$

Which of the following acts as both an oxidizing and a reducing agent?

Which of the following reactions are disproportionation reactions?
$(a)$ $2 Cu^{+} \rightarrow Cu^{2+} + Cu^{0}$
$(b)$ $3 MnO_{4}^{2-} + 4 H^{+} \rightarrow 2 MnO_{4}^{-} + MnO_{2} + 2 H_{2}O$
$(c)$ $2 KMnO_{4} \xrightarrow{\Delta} K_{2}MnO_{4} + MnO_{2} + O_{2}$
$(d)$ $2 MnO_{4}^{-} + 3 Mn^{2+} + 2 H_{2}O \rightarrow 5 MnO_{2} + 4 H^{+}$
Select the correct option from the following:

Assign $A, B, C, D$ from the given type of reaction.
$H_3PO_3 \xrightarrow{\Delta} H_3PO_4 + PH_3 \uparrow$