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

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.

6370g

To determine the amount of sulfuric acid (H2SO4) that can be prepared from a given number of moles of sulfur (S), we need to use the balanced chemical equation for the reaction:

S + O2 → SO2 (Eq. 1)
2 SO2 + O2 → 2 SO3 (Eq. 2)
SO3 + H2O → H2SO4 (Eq. 3)

First, let's calculate the number of moles of sulfur dioxide (SO2) produced from the given amount of sulfur:

Using Eq. 1, we have:
1 mole of sulfur produces 1 mole of sulfur dioxide.
Therefore, 37 moles of sulfur will produce 37 moles of sulfur dioxide.

Next, we calculate the number of moles of sulfur trioxide (SO3) produced from the sulfur dioxide:

Using Eq. 2, we have:
2 moles of sulfur dioxide produce 2 moles of sulfur trioxide.
Therefore, 37 moles of sulfur dioxide will produce 37 moles of sulfur trioxide.

Finally, we calculate the number of moles of sulfuric acid (H2SO4) that can be produced from the sulfur trioxide:

Using Eq. 3, we have:
1 mole of sulfur trioxide produces 1 mole of sulfuric acid.
Therefore, 37 moles of sulfur trioxide will produce 37 moles of sulfuric acid.

To convert moles of sulfuric acid into grams, we need to know the molar mass of H2SO4. The molar mass of H2SO4 is:
2(1.01 g/mol for hydrogen) + 32.07 g/mol for sulfur + 4(16.00 g/mol for oxygen) = 98.09 g/mol.

Finally, we calculate the mass of sulfuric acid that can be prepared from 37 moles of sulfur:

Mass = Number of moles × Molar mass
Mass = 37 moles × 98.09 g/mol

Now, you can calculate the final answer by multiplying these values together.