Please answer this chem problem for me?

Question

Consider the following unbalanced equation
Ca3(PO4)2(s) + H2SO4(aq)------> CaSO4(s) + H3PO4(aq)

What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4 by mass)?

Answer 1

Here's the how you do it.

Balance the equation. Element by element.

That gives you the mole ratios of the various compounds.

Convert the moles to mass using the molecular weight of each of the compounds.

That gives you the mass ratios of the various items.

Divide both sides of the equation by the largest mass on the left side of the equation, Then you will have the mass of products per Kg of the at least one of the reactants. Remember you are starting with 1.0 kg of one item and 0.98 of the other.

so you must check to see which reactant will limit the production.

Should be a simple matter of working out the ratios.

Answer 2

Ca3(PO4)2(s) + 3H2SO4(aq) -----> 3CaSO4(S) + 2H3PO4(aq)
Mr of Ca3(PO4)2 = 310.182
therefore no. of moles of Ca3(PO4)2 = 1000/310.182 = 3.224

Mr of H2SO4 = 98
mass of H2SO4 in reaction = 98% * 1kg = 980g
therefore no of moles of H2SO4 in reaction = 10

therefore limiting reagent is Ca3(PO4)2

No of moles of CaSO4 produced = 3.224 *3
No of moles of H3PO4 produced = 3.224 *2

therefore mass of CaSO4 produced = Mr of CaSO4 * 3.224*3 =1316.15g
mass of H3PO4 produced = Mr of H3PO4 *3.224*2
=631.736g