What are the products of this reaction? $S_{s} + 2 H_{2} S O_{4 (a q)} \to$ $S_(s) + 2H_2SO_(4(aq)) ->$

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What are the products of this reaction? $S_{s} + 2 H_{2} S O_{4 (a q)} \to$ $S_(s) + 2H_2SO_(4(aq)) ->$

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Answer 1 · 2017-08-16T11:11:33

We could invoke a comproportionation reaction........

Explanation:

$S_8(s) + 16H_2SO_4(l) → 24SO_2(g) + 16H_2O(l)$

And thus we start with $stackrel(0)S$ and $stackrel(+VI)S$ , and we finish with $stackrel(+IV)S$ . Elemental sulfur is oxidized, and the sulfuric acid is REDUCED. Is it balanced?

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What are the products of this reaction? $S_{s} + 2 H_{2} S O_{4 (a q)} \to$ $S_(s) + 2H_2SO_(4(aq)) ->$

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What are the products of this reaction? S_(s) + 2H_2SO_(4(aq)) ->Ss+2H2SO4(aq)→S_(s) + 2H_2SO_(4(aq)) ->

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What are the products of this reaction? $S_{s} + 2 H_{2} S O_{4 (a q)} \to$ $S_(s) + 2H_2SO_(4(aq)) ->$