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.$A) \, P_4 + OH^{-} 	o PH_3 + H_

Vedclass · Accepted Answer

$2KClO_3 	o 2KCl + 3O_2$

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(D) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced.$A) \, P_4 + OH^{-} 	o PH_3 + H_2PO_2^-$: Phosphorus $(P)$ is oxidized and reduced. This is a disproportionation reaction.$B) \, Cl_2 + OH^{-} 	o Cl^{-} + ClO^-$: Chlorine $(Cl)$ is oxidized and reduced. This is a disproportionation reaction.$C) \, Br_2 + OH^{-} 	o Br^{-} + BrO_3^-$: Bromine $(Br)$ is oxidized and reduced. This is a disproportionation reaction.$D) \, 2KClO_3 	o 2KCl + 3O_2$: Here,chlorine is reduced from $+5$ to $-1$ oxidation state,while oxygen is oxidized from $-2$ to $0$ oxidation state. Since two different elements are undergoing oxidation and reduction,it is not a disproportionation reaction.

Which of the following is not a disproportionation reaction?

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