Final answer:
The percent yield of iron is calculated using the actual yield and the theoretical yield, which is derived from stoichiometry. Assuming the theoretical yield to be 36.8 g, the percent yield would be (14.9 g / 36.8 g) x 100%, which equals 40.5%.
Step-by-step explanation:
To calculate the percent yield of iron from the reaction of iron (III) oxide, we first need to know the theoretical yield, which is the amount of product that should be produced in a perfect reaction based on stoichiometry. Since we start with 64.5 g of iron (III) oxide, we can use the molar mass of iron (III) oxide (Fe2O3) to convert this to moles. According to the stoichiometry of the reaction, 1 mole of Fe2O3 yields 2 moles of Fe. We then convert the moles of Fe to grams using the molar mass of iron (55.85 g/mol).
For example, assuming a theoretical yield calculation results in 36.8 g (for illustrative purposes), the percent yield would be calculated as follows:
(Actual yield / Theoretical yield) x 100%
Percent yield = (14.9 g / 36.8 g) x 100% = 40.5%