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Will this reaction proceed under standard conditions? I don't really care if it is quite slow, as long as it takes less than a month to finish:

$$\ce{S8(s) + 24 H2O2(aq) -> 8 H2SO4(aq) + 16 H2O(l)}$$

My rationale for this happening is that the elemental sulfur can be oxidized by hydrogen peroxide to form sulfur dioxide, which is further oxidized by hydrogen peroxide to form sulfur trioxide. This then reacts with water to form sulfuric acid.

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  • $\begingroup$ I expect it to be thermodynamically feasible, but quite slow. $\endgroup$ – Ivan Neretin Jun 25 '16 at 14:29
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You will likedly find it faster to perform the first oxidation by burning the elemental sulphur in a little tinfoil boat to produce gaseous sulphur dioxide. then set up some aperatus sucking the gasses produced to bubble up through the hydrogen peroxide to produce sulphuric acid. The peroxide does not oxidize sulphur dioxide to sulphur trioxide because it forms sulphuric acid directly.

Does require some aperatus but will be much faster than waiting for the peroxide. Calculate the gibs free energy if you are not sure if a reaction will be spontaneous.

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    $\begingroup$ To quote sulfur dioxide's Wikipedia page directly: "Inhaling sulfur dioxide is associated with increased respiratory symptoms and disease, difficulty in breathing, and premature death." $\endgroup$ – ringo Sep 13 '16 at 8:57
  • $\begingroup$ @ringo Of course, dealing with corrosive or toxic gases should be performed in a fume hood or with some kind of respirator. $\endgroup$ – sadljkfhalskdjfh Sep 15 '16 at 2:45

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