Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
For the end of this problem I keep getting 2.71596.
Do I always have to divide the top number by the bottom? In this case... 1mol divided by 174.1g of juglone?
![### Calculating Molar Mass I
Juglone, a dye known for centuries, is produced from the husks of black walnuts. It is also a natural herbicide (weed killer) that kills off competitive plants around the black walnut tree but does not affect grass and other noncompetitive plants. The formula for juglone is \( \text{C}_{10}\text{H}_{6}\text{O}_{3} \).
#### Tasks:
a. Calculate the molar mass of juglone.
b. A sample of \( 1.56 \times 10^{-2} \) g of pure juglone was extracted from black walnut husks. How many moles of juglone does this sample represent?
---
### Solution
#### a. Calculation of Molar Mass:
The molar mass is obtained by summing the masses of the component atoms. In 1 mole of juglone, there are 10 moles of carbon atoms, 6 moles of hydrogen atoms, and 3 moles of oxygen atoms:
- Carbon (C):
\[
10 \, \text{C}: \quad 10 \times 12.01 \, \text{g} = 120.1 \, \text{g}
\]
- Hydrogen (H):
\[
6 \, \text{H}: \quad 6 \times 1.008 \, \text{g} = 6.048 \, \text{g}
\]
- Oxygen (O):
\[
3 \, \text{O}: \quad 3 \times 16.00 \, \text{g} = 48.00 \, \text{g}
\]
Mass of 1 mole of \( \text{C}_{10}\text{H}_{6}\text{O}_{3} \):
\[
120.1 \, \text{g} + 6.048 \, \text{g} + 48.00 \, \text{g} = 174.1 \, \text{g}
\]
The mass of 1 mole of juglone is 174.1 g, which is the molar mass.
#### b. Determination of Moles in a Sample:
The mass of 1 mole of this compound is 174.1 g; thus, \( 1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F40e25f29-5021-499e-9c49-7da7bd92383c%2F89bb68ea-1954-4c5a-a190-7a7cfe3489cf%2F8nf2bpe.png&w=3840&q=75)
Transcribed Image Text:### Calculating Molar Mass I
Juglone, a dye known for centuries, is produced from the husks of black walnuts. It is also a natural herbicide (weed killer) that kills off competitive plants around the black walnut tree but does not affect grass and other noncompetitive plants. The formula for juglone is \( \text{C}_{10}\text{H}_{6}\text{O}_{3} \).
#### Tasks:
a. Calculate the molar mass of juglone.
b. A sample of \( 1.56 \times 10^{-2} \) g of pure juglone was extracted from black walnut husks. How many moles of juglone does this sample represent?
---
### Solution
#### a. Calculation of Molar Mass:
The molar mass is obtained by summing the masses of the component atoms. In 1 mole of juglone, there are 10 moles of carbon atoms, 6 moles of hydrogen atoms, and 3 moles of oxygen atoms:
- Carbon (C):
\[
10 \, \text{C}: \quad 10 \times 12.01 \, \text{g} = 120.1 \, \text{g}
\]
- Hydrogen (H):
\[
6 \, \text{H}: \quad 6 \times 1.008 \, \text{g} = 6.048 \, \text{g}
\]
- Oxygen (O):
\[
3 \, \text{O}: \quad 3 \times 16.00 \, \text{g} = 48.00 \, \text{g}
\]
Mass of 1 mole of \( \text{C}_{10}\text{H}_{6}\text{O}_{3} \):
\[
120.1 \, \text{g} + 6.048 \, \text{g} + 48.00 \, \text{g} = 174.1 \, \text{g}
\]
The mass of 1 mole of juglone is 174.1 g, which is the molar mass.
#### b. Determination of Moles in a Sample:
The mass of 1 mole of this compound is 174.1 g; thus, \( 1
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY