If the theoretical yield of Fe in a reaction is 10.0 g and 8.88 g of Fe was actually obtained, what is the percent yield of Fe?

• A. 112.6%
• B. 8.88%
• C. 80.0%
• D. 88.8%

Answer: (D)

Verified step by step guidance

1. Identify the given values: the theoretical yield of Fe is 10.0 g, and the actual yield obtained is 8.88 g.
2. Recall the formula for percent yield, which compares the actual yield to the theoretical yield: \(\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%\).
3. Substitute the given values into the formula: \(\text{Percent Yield} = \left( \frac{8.88\ \text{g}}{10.0\ \text{g}} \right) \times 100\%\).
4. Perform the division inside the parentheses to find the ratio of actual to theoretical yield (do not calculate the final number here, just set up the expression).
5. Multiply the ratio by 100 to convert it to a percentage, which will give the percent yield of Fe.