Question #82a89

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Question #82a89

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Answer 1 · 2016-06-20T19:15:58

I think you need to research the [contact process.](https://en.wikipedia.org/wiki/Contact_process)

Explanation:

AFAIK, elemental sulfur is oxidized stepwise to give $S O_{3}$ $SO_3$ :

$S (s) + O_{2} (g) \to S O_{2} (g)$ $S(s) +O_2(g)rarrSO_2(g)$

$2 S O_{2} (g) + O_{2} (g) \to 2 S O_{3} (g)$ $2SO_2(g) + O_2(g) rarr 2SO_3(g)$

The sulfur trioxide could be directly treated with water to give $H_{2} S O_{4}$ $H_2SO_4$ . I have seen a couple of plants, and it is an incredibly dirty and smelly process. Of course, both oxidations are catalyzed; I think supported $V_{2} O_{5}$ $V_2O_5$ is the catalyst of choice.

One thing the reaction has got going for it, is that both oxidations are exothermic. Sulfur trioxide may be directly converted to sulfuric acid:

$S O_{3} (g) + H_{2} O (g) \to H_{2} S O_{4} (a q)$ $SO_3(g) + H_2O(g) rarr H_2SO_4(aq)$

But this opens another can of worms. Usually sulfuric acid is reacted directly with sulfur trioxide to give oleum, $H_{2} S_{2} O_{7}$ $H_2S_2O_7$ , which is the feedstock for $H_{2} S O_{4}$ $H_2SO_4$ .

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Question #82a89

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