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March 29, 2017

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Sulfuric acid (H2SO4) is prepared commercially from elemental sulfur using the contact
process. In a typical sequence of reactions,
the sulfur is first burned:
S + O2 → SO2 ,
then it is converted to SO3 using a catalyst:
2 SO2 + O2 → 2 SO3 .
The resulting SO3 is reacted with water to
produce the desired product:
SO3 + H2O → H2SO4 .
How much sulfuric acid could be prepared
from 37 moles of sulfur?
Answer in units of g

  • chemistry - ,

    look at the final formula. H2SO4

    for each mole of S, there is one mole of H2SO4

    so the answer is 37 moles of H2SO4.

  • chemistry - ,

    6370g

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