Final answer:
To calculate the percent yield, the theoretical yield must be calculated from the balanced chemical equation and the amount of reactants used. Due to discrepancies and lack of complete information, the exact calculation of percent yield cannot be provided. However, the process involves stoichiometric calculations, converting grams to moles, and using the percent yield formula.
Step-by-step explanation:
Calculating Percent Yield in a Chemical Reaction
The question at hand involves a chemical reaction between iron (III) phosphate and sodium sulfate, where iron (III) sulfate and sodium phosphate are produced. The concept being addressed is percent yield, which is a measure of the efficiency of a chemical reaction.
To calculate percent yield, you need to know the theoretical yield, which can be calculated from the balanced chemical equation and the amount of reactants used. In this case, we have 27.0 g of iron (III) phosphate reacting. Through stoichiometry, we can find out how many grams of iron (III) sulfate are expected to be produced theoretically from those 27.0 g. However, since the actual amount produced was 18.75 g, we calculate percent yield using the formula:
Percent Yield = (Actual Yield / Theoretical Yield) x 100
First, we cannot calculate the theoretical yield without the balanced chemical equation. The provided information has some discrepancies, for instance, the compound iron(II) phosphate is mentioned, but this does not match the reactant in question, which is supposed to be iron(III) phosphate. Additionally, the given reactions do not match the one we are discussing, so we assume the relevant equation is as follows:
FePO4 + 3 Na2SO4 → Fe2(SO4)3 + 2 Na3PO4
Using stoichiometric calculations, you would then determine the number of moles of iron (III) phosphate and convert them to moles of iron (III) sulfate, using the molar masses of both compounds. Next, you would convert the moles of iron (III) sulfate to grams, giving you the theoretical yield. Finally, by inserting the actual yield and theoretical yield into the percent yield formula, you would calculate the percent yield. Since the correct stoichiometric calculations are not provided, we cannot complete the calculation.
It is also important to consider significant figures in your final answer, as it reflects the precision of your measurements and calculations.