To calculate the percentage yield of iron(III) chloride (FeCl3), we need to follow these steps:
1. Identify the actual yield: The actual yield is the mass of FeCl3 that was actually produced during the reaction. According to the information given, the actual mass of FeCl3 produced is 24.3 grams.
2. Identify the theoretical yield: The theoretical yield is the maximum possible mass of FeCl3 that could be produced in the reaction, based on stoichiometric calculations. Here, it is assumed that the theoretical mass of FeCl3 is 28.0 grams.
3. Use the percentage yield formula:
[tex]\[
\text{Percentage Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100
\][/tex]
Plugging in the actual yield and the theoretical yield:
[tex]\[
\text{Percentage Yield} = \left( \frac{24.3}{28.0} \right) \times 100
\][/tex]
4. Calculate the percentage yield:
[tex]\[
\text{Percentage Yield} = 86.79\%
\][/tex]
So, the percentage yield of the iron(III) chloride (FeCl3) produced in this reaction is approximately 86.79%.
