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Non- STP Stoichiometry... help!?
This is a question from a set of problems I am doing and I am stuck on what to do....
One of the major commercial uses of sulfuric acid is in the production of phosphoric acid and calcium sulfate. What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg of calcium phosphate and 1.0kg of concentrated sulfuric acid (98% sulfuric acid by mass)?
Please reveiw the use of M (molarity)
please show as much work as possible (with things labeled) because I want to follow along and see exactly how you got the answer.
Thank you!
Dr. A... there was no other info that I was given. That was the entire question and we were soposed to answer it based on that disription...
1 Answer
- Dr.ALv 71 decade agoFavorite Answer
Ca3(PO4)2 + 3H2SO4 >>2 H3PO4 + 3CaSO4
is the balanced equation
Moles Ca3(PO4)2 = 1000 g / 310.18 g/mol =3.22
Now we must get the molar concentration of H2SO4 .
To get it we must know the density in g/L
density x 98 / 100 = g/L
divide by molar mass of H2SO4 and you have the molarity.
If you tell me at once the density I will answer you
