Question

question specifies that we got 1.88×1023 dioxygen molecules...i.e. a molar quantity of...

1.88×1023⋅molecules6.022×1023⋅molecules⋅mol−1=0.312⋅mol...

But we gots with respect to sulfur, 6.67⋅g32.06⋅g⋅mol−1=0.208⋅mol...

And a bit of arithmetic later, we establish that we got stoichiometric quantities of dioxygen, and sulfur….in the reaction we produce a mass of ………..

0.208⋅mol×80.07⋅g⋅mol−1=16.65⋅g.

Note that when sulfur trioxide is made industrially (and this a very important commodity chemical), sulfur is oxidized to SO2, and this is then oxidized up to SO3with some catalysis...

SO2(g)+12O2(g)V2O5−−→SO3(g)

SO3(g)+H2O(l)→H2SO4(aq)sulfuric acid

The industrial sulfur cycle must be a dirty, smelly, unfriendly process. The process is undoubtedly necessary to support our civilization....​

Answer 1

Answer:

jajsxusvejj955-5*5 31616643431699* *%+%9+6