Question

Write the equation for the reaction of iron (iii) phosphate with sodium sulfate tomake iron (iii) sulfate and sodium phosphate.

a. if you perform this reaction with 25 grams of iron (iii) phosphate and an excessof sodium sulfate, how many grams of iron (iii) sulfate can you make?
b. If 18.5 grams of iron (III) sulfate are actually made when I do this reaction, what is my percent yield?
c. Is the answer from problem #1 reasonable? Explain.
d. If I do this reaction with 15 grams of sodium sulfate and get a 65.0% yield, how many grams of sodium phosphate will I make?

Answer 1

The reaction of iron(III) phosphate with sodium sulfate forms iron(III) sulfate and sodium phosphate. Calculating the theoretical and actual yields, as well as the percent yield, requires stoichiometric conversions and applying the formula for percent yield. For sodium phosphate production, the yield is determined using the stoichiometry of the reaction and applying the given percent yield.

Step-by-step explanation:

Chemical Reaction Equation

The balanced chemical equation for the reaction of iron (III) phosphate with sodium sulfate to form iron (III) sulfate and sodium phosphate is:

FePO4 + 3Na2SO4 → 2Fe2(SO4)3 + 3Na3PO4

a. Theoretical Yield:

To find the theoretical yield of iron (III) sulfate from 25 grams of iron (III) phosphate, we need to follow these steps:

Convert grams of iron (III) phosphate to moles.

Use stoichiometry to find moles of iron (III) sulfate produced.

Convert moles of iron (III) sulfate to grams.

This calculation will involve the molar masses of iron (III) phosphate and iron (III) sulfate, which are not given in the problem and should be obtained from a periodic table.

b. Percent Yield:

The percent yield is calculated using the formula:

Percent Yield = (Actual Yield / Theoretical Yield) × 100%

In this case, with an actual yield of 18.5 grams of iron (III) sulfate, we would substitute the actual yield and the theoretical yield from part a into the equation.

c. Reasonability of Theoretical Yield:

The reasonability of the theoretical yield identified in part a can be assessed after performing the calculation. If the obtained theoretical yield is close to the actual yield, it is considered reasonable. Discrepancies might be due to experimental error or incomplete reactions.

d. Sodium Phosphate Yield:

To find out the yield of sodium phosphate when 15 grams of sodium sulfate are used with a 65.0% yield:

Convert grams of sodium sulfate to moles and use stoichiometry to find moles of sodium phosphate produced.

Apply the percent yield to calculate the actual grams of sodium phosphate.

As before, precise calculations require the molar masses which must be obtained from other sources.