A reaction uses 32.5 g of Zn and produces 28.0 g of ZnCl_2. If the theoretical yield of ZnCl_2 is 40.5 g, what is the percent yield for the reaction?

• A. 127.5%
• B. 87.5%
• C. 69.1%
• D. 44.2%

Answer: (C)

Verified step by step guidance

1. Identify the given quantities: the actual yield of ZnCl_2 is 28.0 g, and the theoretical yield of ZnCl_2 is 40.5 g.
2. Recall the formula for percent yield: \(\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%\).
3. Substitute the given values into the formula: \(\text{Percent Yield} = \left( \frac{28.0\ \text{g}}{40.5\ \text{g}} \right) \times 100\%\).
4. Perform the division inside the parentheses to find the decimal yield (do not calculate the final number here).
5. Multiply the decimal yield by 100 to convert it to a percentage, which gives the percent yield of the reaction.