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(D) The given reaction is $P_4 + 3NaOH + 3H_2O \longrightarrow PH_3 + 3NaH_2PO_2$.In this reaction,the oxidation state of phosphorus $(P)$ changes fro

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$D$

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(D) The given reaction is $P_4 + 3NaOH + 3H_2O \longrightarrow PH_3 + 3NaH_2PO_2$.In this reaction,the oxidation state of phosphorus $(P)$ changes from $0$ in $P_4$ to $-3$ in $PH_3$ and $+1$ in $NaH_2PO_2$.Since the same element is simultaneously oxidized and reduced,this is a disproportionation reaction.None of the categories $A$,$B$,or $C$ describe a redox reaction of this type.Therefore,the correct assignment is $D$ (no reaction among the given categories).

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Assign $A$,$B$,$C$,$D$ from given type of reaction.$A$ for precipitate formation reaction.$B$ for precipitate dissolution reaction.$C$ for precipitate exchange reaction.$D$ for no reaction.$P_4 + 3NaOH + 3H_2O \longrightarrow PH_3 + 3NaH_2PO_2$Identify the correct category for the given reaction.