Chapter 12, Problem 69A

Interpretation Introduction

Interpretation: To calculate the percent yield for the given reaction.

Concept Introduction: Percent yield can be calculated by dividing the actual yield by the theoretical yield multiplied by 100.

  $\text{Percent yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\text{×100\%}$

Answer to Problem 69A

The percent yield is $\text{20}\text{.0\%}$ .

Explanation of Solution

Percent yields involve the actual yield and theoretical yield. It can be calculated by dividing the actual yield by the theoretical yield multiplied by 100. Therefore, a percent yield must be greater than 0% and lesser than 100%.

  $\begin{array}{c}\text{B}\to \text{C}\\ \text{Percent yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\text{×100\%}\\ \text{=}\frac{2.00\text{mol C}}{4.00\text{ mol C}}\times 100\%\\ =30.0\%\end{array}$

Let $x$ represents the actual yield of compound D.

  $\begin{array}{c}\text{Percent yield}=\text{25}\text{.0\%}\\ \text{=}\frac{x}{\text{2 mol D}}\times 100\%\\ x=0.250\times \text{2 mol D}\\ x=0.500\text{ mol D}\end{array}$

Let $y$ represents the actual yield of compound E.

  $\begin{array}{c}\text{Percent yield}=10.\text{0\%}\\ \text{=}\frac{y}{\text{0}\text{.500 mol E}}\times 100\%\\ y=0.100\times \text{0}\text{.500 mol E}\\ y=0.0500\text{ mol E}\end{array}$

  $\begin{array}{c}\text{E}\to \text{F}\\ \text{Percent yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\text{×100\%}\\ \text{=}\frac{0.0100\text{mol F}}{\text{0}\text{.0500 mol F}}\times 100\%\\ =20.0\%\end{array}$

Conclusion

Thus, the percent yield is $\text{20}\text{.0\%}$ .