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

I worked this for Chasm several days ago. Here is a link.

http://www.jiskha.com/display.cgi?id=1346951916
Let me know if anything isn't clear.

To determine the amount of sulfuric acid that can be prepared from 63 moles of sulfur, we need to calculate the molar mass of sulfuric acid (H2SO4) and then use stoichiometry to convert moles of sulfur to grams of sulfuric acid.

1. Calculate the molar mass of sulfuric acid (H2SO4):
- Molar mass of 2 hydrogen atoms (H): 2 g/mol × 2 = 4 g/mol
- Molar mass of 1 sulfur atom (S): 32 g/mol
- Molar mass of 4 oxygen atoms (O): 16 g/mol × 4 = 64 g/mol
- Total molar mass of sulfuric acid (H2SO4): 4 g/mol + 32 g/mol + 64 g/mol = 98 g/mol

2. Determine the molar ratio between sulfur (S) and sulfuric acid (H2SO4) from the balanced chemical equation:
- From the equation: 1 mole of sulfur (S) reacts to produce 1 mole of sulfuric acid (H2SO4)

3. Convert moles of sulfur to grams of sulfuric acid:
- Multiply the number of moles of sulfur (63 moles) by the molar mass of sulfuric acid (98 g/mol):
63 moles × 98 g/mol = 6174 g

Therefore, 63 moles of sulfur can be converted into 6174 grams of sulfuric acid.