0.573 g of calcium chloride reacts with excess of 0.5 M Na3PO4 to form .523 g of isolated calcium phosphate precipitate.

Determine theoretical yield, actual yield, and percent yield for this reaction.

To determine the theoretical yield, actual yield, and percent yield for the given reaction, we need to utilize stoichiometry and the balanced chemical equation of the reaction.

1. Find the balanced chemical equation for the reaction:
CaCl2 + 2Na3PO4 --> 3Ca3(PO4)2 + 6NaCl

2. Calculate the moles of calcium chloride (CaCl2):
Given mass of calcium chloride = 0.573 g, molar mass of CaCl2 = 110.98 g/mol
Moles of CaCl2 = mass / molar mass = 0.573 g / 110.98 g/mol = 0.00516 mol (rounded to 5 decimal places)

3. Determine the limiting reactant:
To determine the limiting reactant, compare the moles of calcium chloride with the moles of sodium phosphate (Na3PO4), taking into account the stoichiometry of the reaction. From the balanced equation, the stoichiometry of CaCl2 to Na3PO4 is 1:2.
Hence, the moles of Na3PO4 = 2 * moles of CaCl2 = 2 * 0.00516 mol = 0.01032 mol (rounded to 5 decimal places)

Since the moles of Na3PO4 (0.01032 mol) are in excess compared to the moles of CaCl2 (0.00516 mol), CaCl2 is the limiting reactant.

4. Calculate the moles of calcium phosphate precipitate (Ca3(PO4)2):
From the balanced equation, the stoichiometry of CaCl2 to Ca3(PO4)2 is 1:3.
Hence, moles of Ca3(PO4)2 = 3 * moles of CaCl2 = 3 * 0.00516 mol = 0.01548 mol (rounded to 5 decimal places)

5. Determine the theoretical yield:
The theoretical yield represents the maximum amount of product that can be obtained according to the balanced equation.
Given the molar mass of Ca3(PO4)2 = 310.18 g/mol
Theoretical yield = moles of Ca3(PO4)2 * molar mass of Ca3(PO4)2 = 0.01548 mol * 310.18 g/mol = 4.802 g (rounded to 3 decimal places)

6. Calculate the actual yield:
Given mass of isolated calcium phosphate precipitate = 0.523 g

7. Determine the percent yield:
Percent yield is calculated by dividing the actual yield by the theoretical yield and multiplying the result by 100.
Percent yield = (actual yield / theoretical yield) * 100
Percent yield = (0.523 g / 4.802 g) * 100 = 10.89% (rounded to 2 decimal places)

In summary,
Theoretical yield: 4.802 g
Actual yield: 0.523 g
Percent yield: 10.89%

nevermind I figured it out