Which of the following is not a disproportion | vedclass

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(D) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.In option $A$,$Hg_2Cl_2$ undergoe

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$BaO_2 + H_2SO_4 \longrightarrow BaSO_4 + H_2O_2$

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(D) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.In option $A$,$Hg_2Cl_2$ undergoes disproportionation where $Hg$ is oxidized from $+1$ to $+2$ and reduced from $+1$ to $0$.In option $B$,$H_3PO_3$ undergoes disproportionation where $P$ is oxidized from $+3$ to $+5$ and reduced from $+3$ to $-3$.In option $C$,$Cl_2$ undergoes disproportionation where $Cl$ is oxidized from $0$ to $+1$ and reduced from $0$ to $-1$.In option $D$,$BaO_2 + H_2SO_4 \longrightarrow BaSO_4 + H_2O_2$ is a double displacement reaction,not a redox reaction,as there is no change in oxidation states of any element.

Which of the following is not a disproportionation reaction?

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