H_2S (5 moles) reacts completely with acidifi | vedclass

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(B) The balanced chemical equation for the reaction is: $2 KMnO_4 + 5 H_2S + 3 H_2SO_4 \rightarrow K_2SO_4 + 2 MnSO_4 + 5 S + 8 H_2O$ For $5$ moles of

Vedclass · Accepted Answer

$18$

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(B) The balanced chemical equation for the reaction is: $2 KMnO_4 + 5 H_2S + 3 H_2SO_4 ightarrow K_2SO_4 + 2 MnSO_4 + 5 S + 8 H_2O$ For $5$ moles of $H_2S$,the stoichiometry remains the same as in the balanced equation. Thus,$x = 8$ moles of $H_2O$ are produced. In this redox reaction,$S^{2-}$ is oxidized to $S^0$ (loss of $2$ electrons per $H_2S$ molecule). For $5$ moles of $H_2S$,the total electrons involved $y = 5 	imes 2 = 10$. Therefore,$(x + y) = 8 + 10 = 18$.

$H_2S$ ($5$ moles) reacts completely with acidified aqueous potassium permanganate solution. In this reaction,the number of moles of water produced is $x$,and the number of moles of electrons involved is $y$. The value of $(x+y)$ is. . . . . .

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