The reaction H_3PO_2 xrightarrow{Delta} (X) + | vedclass

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(C) The reaction is: $3 H_3PO_2 \xrightarrow{\Delta} 2 H_3PO_3 + PH_3$ and $4 H_3PO_2 \xrightarrow{\Delta} 3 H_3PO_4 + PH_3$. In this reaction,the oxi

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Disproportionation reaction

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(C) The reaction is: $3 H_3PO_2 \xrightarrow{\Delta} 2 H_3PO_3 + PH_3$ and $4 H_3PO_2 \xrightarrow{\Delta} 3 H_3PO_4 + PH_3$. In this reaction,the oxidation state of phosphorus in $H_3PO_2$ is $+1$. In $PH_3$,the oxidation state is $-3$ (reduction),and in $H_3PO_3$ or $H_3PO_4$,the oxidation state is $+3$ or $+5$ respectively (oxidation). Since the same element is simultaneously oxidized and reduced,it is a disproportionation reaction.

The reaction $H_3PO_2 \xrightarrow{\Delta} (X) + PH_3$ is a:

Similar Questions

Which one of the following does not undergo disproportionation reaction?

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$H_2O_2 \xrightarrow{R.T} H_2O + \frac{1}{2} O_2$

In the following reaction,$3Br_2 + 6CO_3^{2-} + 3H_2O \rightarrow 5Br^{-} + BrO_3^- + 6HCO_3^-$,what happens to bromine?

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This reaction is an example of -

An example of a disproportionation reaction is

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