Sulfuric acid (H2SO4) is prepared commer-

cially 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 63 moles of sulfur?
Answer in units of g

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To calculate the amount of sulfuric acid that could be prepared from 63 moles of sulfur, we need to determine the molar mass of sulfuric acid (H2SO4).

The molar mass of sulfuric acid can be calculated by summing the atomic masses of its constituent elements:
H (hydrogen) has an atomic mass of 1 g/mol,
S (sulfur) has an atomic mass of 32.06 g/mol, and
O (oxygen) has an atomic mass of 16 g/mol.

So, the molar mass of H2SO4 is:
(2 * 1 g/mol) + (1 * 32.06 g/mol) + (4 * 16 g/mol) = 98.08 g/mol.

Now, to calculate the amount of sulfuric acid that can be prepared, we need to convert moles of sulfur to moles of sulfuric acid using stoichiometry.

From the given reaction equations, we can see that 1 mole of sulfur reacts to form 1 mole of sulfuric acid.

Therefore, the amount of sulfuric acid that can be prepared from 63 moles of sulfur is also 63 moles.

Finally, to convert moles of sulfuric acid to grams, we multiply the number of moles by the molar mass of sulfuric acid:

63 moles * 98.08 g/mol = 6174.24 g.

Therefore, 63 moles of sulfur can produce 6174.24 grams of sulfuric acid.