Fundamental Of Chemical Engineering
posted by NONO on .
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: