Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 112

A reaction having a 90 percent yield may be considered a successful experiment. However, in the synthesis of complex molecules such as chlorophyll and many anticancer drugs, a chemist often has to carry out multiple-step synthesis. What is the overall percent yield for such a synthesis, assuming it is a 30 -step reaction with a 90 percent yield at each step?

Short Answer

Expert verified
The overall yield percentage for a 30-step reaction with a 90 percent yield at each step is approximately 4.24 percent

Step by step solution

01

Understand the Problem

The problem is asking for the overall yield of a 30 step reaction, where each step has a 90 percent success rate. With multistep reactions, the yield from one step is used as the starting material for the next, so understanding the decrease in yield at each stage is crucial to solving the problem.
02

Determine the Yield at Each Step

The yield at each step is given as 90 percent, or 0.90 when expressed as a decimal. This means that 90 percent of the material from one step is successfully used in the next step.
03

Calculate the Overall Yield

To calculate the overall yield, multiply the yield of each step. Since there are 30 steps and the yield at each step is 0.90, the overall yield is \(0.90^{30}\).
04

Convert to Percentage

To convert the decimal to a percentage, multiply the result by 100. Therefore, the overall yield percentage is \(0.90^{30} \times 100\).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Carbohydrates are compounds containing carbon, hydrogen, and oxygen in which the hydrogen to oxygen ratio is 2: 1 . A certain carbohydrate contains 40.0 percent carbon by mass. Calculate the empirical and molecular formulas of the compound if the approximate molar mass is \(178 \mathrm{~g}\).

Propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) is a component of natural gas and is used in domestic cooking and heating. (a) Balance the following equation representing the combustion of propane in air: $$ \mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} $$ (b) How many grams of carbon dioxide can be produced by burning 3.65 moles of propane? Assume that oxygen is the excess reagent in this reaction.

What is an atomic mass unit? Why is it necessary to introduce such a unit?

What are the empirical formulas of the compounds with the following compositions? (a) 40.1 percent \(\mathrm{C}\) 6.6 percent \(\mathrm{H}, 53.3\) percent \(\mathrm{O}\) (b) 18.4 percent \(\mathrm{C}\) 21.5 percent \(\mathrm{N}, 60.1\) percent \(\mathrm{K}\)

Describe the steps involved in the mole method.
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free