Which of the following is only a redox reacti | vedclass

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Question

(D) disproportionation reaction is a type of redox reaction where the same element in a single oxidation state is simultaneously oxidized and reduced.

Vedclass · Accepted Answer

$P_4 + 8 SOCl_2 \rightarrow 4 PCl_3 + 2 S_2 Cl_2 + 4 SO_2$

Vedclass · Answer

(D) disproportionation reaction is a type of redox reaction where the same element in a single oxidation state is simultaneously oxidized and reduced.In option $A$, $P$ in $H_3 PO_3$ $(+3)$ is oxidized to $H_3 PO_4$ $(+5)$ and reduced to $PH_3$ $(-3)$.In option $B$, $O$ in $H_2 O_2$ $(-1)$ is oxidized to $O_2$ $(0)$ and reduced to $H_2 O$ $(-2)$.In option $C$, $P$ in $P_4$ $(0)$ is oxidized to $NaH_2 PO_2$ $(+1)$ and reduced to $PH_3$ $(-3)$.In option $D$, $P$ in $P_4$ $(0)$ is oxidized to $PCl_3$ $(+3)$ and $S$ in $SOCl_2$ $(+4)$ is reduced to $S_2 Cl_2$ $(+1)$. Since different elements undergo oxidation and reduction, it is a redox reaction but not a disproportionation reaction.

Which of the following is only a redox reaction but not a disproportionation reaction?

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