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 17 moles of sulfur?
Answer in units of g
FOURTEEN questions in 4 minutes! Wow ... I think that's some kind of record!! And not a question among them!
I'm removing all but this one, and when you decide to follow directions and post YOUR QUESTIONS (not your assignments), with your thoughts included, someone may be happy to help.
To determine the amount of sulfuric acid that can be prepared from 17 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):
- Atomic mass of hydrogen (H) = 1 g/mol
- Atomic mass of sulfur (S) = 32.07 g/mol
- Atomic mass of oxygen (O) = 16 g/mol
Molar mass of sulfuric acid (H2SO4) = (2 * 1) + 32.07 + (4 * 16) = 98.09 g/mol
2. Use stoichiometry to convert moles of sulfur to moles of sulfuric acid:
- From the balanced equation, we know that 1 mole of sulfur reacts with 1 mole of sulfuric acid.
- Therefore, the moles of sulfuric acid produced is equal to the moles of sulfur used.
3. Convert moles of sulfuric acid to grams of sulfuric acid:
- Multiply the moles of sulfuric acid by the molar mass of sulfuric acid to get the mass in grams.
Mass of sulfuric acid = Moles of sulfuric acid * Molar mass of sulfuric acid
Let's calculate it:
Molar mass of sulfuric acid = 98.09 g/mol
Moles of sulfuric acid = Moles of sulfur = 17 mol
Mass of sulfuric acid = 17 mol * 98.09 g/mol
Mass of sulfuric acid = 1666.53 g
Therefore, 17 moles of sulfur can produce 1666.53 grams of sulfuric acid.