If salt Q undergoes a redox reaction with H_2 | vedclass

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(D) In an acidic medium,the permanganate ion $(MnO_4^-)$ acts as a strong oxidizing agent and $H_2S$ acts as a reducing agent.The balanced redox react

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Both $(A)$ and $(C)$

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(D) In an acidic medium,the permanganate ion $(MnO_4^-)$ acts as a strong oxidizing agent and $H_2S$ acts as a reducing agent.The balanced redox reaction is: $2MnO_4^- + 5H_2S + 6H^+ \rightarrow 2Mn^{2+} + 5S + 8H_2O$.In this reaction,$Mn$ is reduced to $Mn^{2+}$ and $S^{2-}$ is oxidized to $S$.Species like $MnO_4^{2-}$ (manganate ion) are stable only in strongly alkaline media,and $MnO_2$ is typically formed in neutral or weakly alkaline media.Therefore,neither $MnO_4^{2-}$ nor $MnO_2$ can be a product in an acidic medium.

If salt $Q$ undergoes a redox reaction with $H_2S$ in an acidic medium,then which of the following species cannot be a possible product?

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