Question

1. if the percent yield of a reaction was 65.0% and its theoretical yield was 0.652 g of what was the actual yield?

Explanation:

Step1: Recall the percent yield formula

The formula for percent yield is: $\text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%$

We need to solve for Actual Yield, so rearrange the formula: $\text{Actual Yield} = \frac{\text{Percent Yield} \times \text{Theoretical Yield}}{100\%}$

Step2: Substitute the given values

Given Percent Yield = $65.0\%$, Theoretical Yield = $0.652\ \text{g}$

Substitute into the formula: $\text{Actual Yield} = \frac{65.0\% \times 0.652\ \text{g}}{100\%}$

First, convert the percentage to a decimal: $65.0\% = 0.650$

Then calculate: $0.650 \times 0.652\ \text{g} = 0.4238\ \text{g}$ (round to appropriate significant figures, here three significant figures as given in percent yield and theoretical yield)

Answer:

The actual yield is $0.424\ \text{g}$ (or $0.4238\ \text{g}$ depending on precision)