P_4 + 3KOH + 3H_2O to PH_3 + 3KH_2PO_2; In th | vedclass

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(C) Assigning oxidation states to phosphorus in the given reaction:$\mathop{P_4}\limits^{0} + 3KOH + 3H_2O 	o \mathop{PH_3}\limits^{-3} + 3KH_2\matho

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Both oxidation and reduction.

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(C) Assigning oxidation states to phosphorus in the given reaction:$\mathop{P_4}\limits^{0} + 3KOH + 3H_2O 	o \mathop{PH_3}\limits^{-3} + 3KH_2\mathop{P}\limits^{+1}O_2$In this reaction,the oxidation state of phosphorus changes from $0$ to $-3$ (reduction) and from $0$ to $+1$ (oxidation).Therefore,phosphorus undergoes both oxidation and reduction,which is a disproportionation reaction.

$P_4 + 3KOH + 3H_2O \to PH_3 + 3KH_2PO_2$; In this reaction,phosphorus undergoes:

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