(B) The chemical equation for the reaction is: $P_4 + 3NaOH + 3H_2O \to PH_3 + 3NaH_2PO_2$In this reaction,the oxidation state of phosphorus changes f

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(B) The chemical equation for the reaction is: $P_4 + 3NaOH + 3H_2O \to PH_3 + 3NaH_2PO_2$In this reaction,the oxidation state of phosphorus changes from $0$ in $P_4$ to $-3$ in $PH_3$ (reduction) and $+1$ in $NaH_2PO_2$ (oxidation).Since the same element is simultaneously oxidized and reduced,this is a disproportionation reaction.

Class 11 Chemistry Redox Reactions Auto oxidation and Disproportionation

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The reaction of white phosphorus with aqueous $NaOH$ gives phosphine along with another phosphorus-containing compound. The reaction is known as:

A
Simple redox reaction
B
Disproportionation reaction
C
Decomposition reaction
D
None

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Class 11

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Redox Reactions

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Auto oxidation and Disproportionation

In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$

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$P_4 + 3NaOH + 3H_2O \to 3NaH_2PO_2 + PH_3$ is an example of

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Nitrous acid was disproportionated to form water,$HNO_3$ and $X$. In another reaction,sodium nitrite was reacted with $H_2SO_4$ to form $NaHSO_4, HNO_3$,water and $Y$. What are $X$ and $Y$ respectively?

MediumAP EAMCET 2018

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The compound that cannot act both as an oxidising and reducing agent is:

MediumJEE MAIN 2020

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Manganese $(VI)$ has the ability to disproportionate in an acidic solution. The difference in oxidation states of the two ions it forms in an acidic solution is $...... .$

MediumJEE MAIN 2022

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The reaction of white phosphorus with aqueous $NaOH$ gives phosphine along with another phosphorus-containing compound. The reaction is known as:

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In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$

$P_4 + 3NaOH + 3H_2O \to 3NaH_2PO_2 + PH_3$ is an example of

Nitrous acid was disproportionated to form water,$HNO_3$ and $X$. In another reaction,sodium nitrite was reacted with $H_2SO_4$ to form $NaHSO_4, HNO_3$,water and $Y$. What are $X$ and $Y$ respectively?

The compound that cannot act both as an oxidising and reducing agent is:

Manganese $(VI)$ has the ability to disproportionate in an acidic solution. The difference in oxidation states of the two ions it forms in an acidic solution is $...... .$

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In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$