Question

A reaction that produced 4.8mg4.8 \mathrm{mg} of taxol, an anticancer drug, is reported to have a yield of 38%38 \%. What was the theoretical yield?

Solution

Verified
Step 1
1 of 2

Use the percent yield equation to calculate the theoretical yield of the reaction.

percent  yield=actual yieldtheoretical yield×100%    theoretical yield=(actual yield)(100%)percent yield=4.8  mg100%38%=13  mg\begin{align*} \mathrm{percent\;yield} &=\dfrac{\text{actual yield}}{\text{theoretical yield}}\times100\%\\\\ \implies\\ \text{theoretical yield}&= \dfrac{\left(\text{actual yield}\right)\left(100\%\right)}{\text{percent yield}}\\ &=\begin{array}{c|c} 4.8\;\mathrm{mg} & 100\%\\ \hline & 38\% \end{array}\\ &= 13\;\mathrm{mg} \end{align*}

Create an account to view solutions

Create an account to view solutions

Recommended textbook solutions

Introduction to Chemical Engineering Thermodynamics 7th Edition by Hendrick Van Ness, J.M. Smith, Michael Abbott

Introduction to Chemical Engineering Thermodynamics

7th EditionISBN: 9780073104454Hendrick Van Ness, J.M. Smith, Michael Abbott
591 solutions
Basic Principles and Calculations in Chemical Engineering 8th Edition by David M. Himmelblau, James B. Riggs

Basic Principles and Calculations in Chemical Engineering

8th EditionISBN: 9780132885485David M. Himmelblau, James B. Riggs
Chemical Reaction Engineering 3rd Edition by Octave Levenspiel

Chemical Reaction Engineering

3rd EditionISBN: 9780471254249 (3 more)Octave Levenspiel
228 solutions
Chemistry for Engineering Students 3rd Edition by Brown

Chemistry for Engineering Students

3rd EditionISBN: 9781285199023 (2 more)Brown
1,047 solutions

More related questions

1/4

1/7