Question

Consider the balanced chemical reaction below. How many grams of CaSO₄ can be produced from 1.00 kg of Ca₃(PO₄)₂ and 1.00 kg of H₂SO₄?

Ca₃(PO₄)₂(s) + 3 H₂SO₄(aq) → 3 CaSO₄(s) + 2 H₃PO₄(aq)

Answer 1

To react with 1.36 mol of H₃PO₄, 2.04 mol of Ca(OH)₂ are required.

Step-by-step explanation:

To find out how many moles of Ca(OH)₂ are required to react with 1.36 mol of H₃PO₄, we need to refer to the balanced chemical equation:

3Ca(OH)₂ + 2H₃PO₄ → Ca3(PO4)₂ + 6H₂O

From the equation, we can see that the molar ratio between Ca(OH)₂ and H₃PO₄ is 3:2.

So, for every 3 moles of Ca(OH)₂, we need 2 moles of H₃PO₄.

Therefore, 1.36 mol of H₃PO₄ requires:

(3/2) x 1.36 mol = 2.04 mol