If a sulfuric acid plant is to produce 10 ton/day of 98% sulfuric acid, How much sulfur is needed, how much air is required and how much water is used?
why don't you at least provide the balanced equation used for industrial production of H2SO4?
In doing so, you will have almost solved the problem.
They didn't give us an equation but I write this, I don't now if it's right or not.
SO3 (g) +H2O (l) → H2SO4 (l)
so, now you know the relative amounts (in moles) of the various compounds.
10 tons of 98% acid is 9.8 tons of H2SO4
convert tons to moles (at 98g/mol)
for each mole of S you need 1.5 moles of O2 and 1 mole of H2O.
Now, if you have to account for the fact that air is not pure O2, then you eed to include that in your calculations.
OK what about if we have all this equations:
H2SO4→ so3+H2O
SO3→ SO2+1\2O2
SO2→ S+O2
To determine the amount of sulfur, air, and water needed to produce 10 tons/day of 98% sulfuric acid in a sulfuric acid plant, we can use stoichiometry and the balanced chemical equation for the reaction that produces sulfuric acid.
The balanced chemical equation for the production of sulfuric acid is:
2S + 3O2 + 2H2O -> 2H2SO4
According to the equation, we need 2 moles of sulfur (S) to produce 2 moles of sulfuric acid (H2SO4).
To calculate the amount of sulfur needed:
- Convert the given amount of sulfuric acid (10 tons/day) to moles:
10 tons * (1000 kg/ton) * (1 kg/32.06 g) * (1 mol/98.09 g) = X moles
Since the reaction ratio is 2 moles of sulfuric acid to 2 moles of sulfur, the amount of sulfur needed will be equivalent to the calculated amount of sulfuric acid:
2 moles sulfur : 2 moles sulfuric acid = X moles sulfur : 10 moles sulfuric acid
Simplifying the equation, we get:
X = 10 moles sulfur
Therefore, 10 moles of sulfur is needed to produce 10 tons/day of 98% sulfuric acid.
Next, let's calculate the amount of air required. According to the balanced chemical equation, we need 3 moles of oxygen (O2) for every 2 moles of sulfur.
To calculate the amount of air required:
- Convert the amount of sulfuric acid (10 tons/day) to moles (as done above): X moles
- Multiply the moles of sulfur by the stoichiometric ratio:
(3 moles O2 / 2 moles S) * X moles sulfur = Y moles O2
Finally, let's determine the amount of water used. According to the balanced equation, we need 2 moles of water (H2O) for every 2 moles of sulfur.
To calculate the amount of water used:
- Convert the amount of sulfuric acid (10 tons/day) to moles (as done above): X moles
- Multiply the moles of sulfur by the stoichiometric ratio:
(2 moles H2O / 2 moles S) * X moles sulfur = Z moles H2O
Therefore, the amount of sulfur needed is 10 moles, the amount of air required is Y moles, and the amount of water used is Z moles.