Chemistry for Today: General, Organic, and Biochemistry
Chemistry for Today: General, Organic, and Biochemistry
9th Edition
ISBN: 9781305960060
Author: Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Textbook Question
Book Icon
Chapter 2, Problem 2.43E

Write three relationships (equalities) based on the mole concept for each of the following elements:

a. beryllium

b. lead

c. sodium

Expert Solution
Check Mark
Interpretation Introduction

(a)

Interpretation:

The three relationships (equalities) based on the mole concept for the given elements are to be stated.

Concept introduction:

Molar mass is the sum of the atomic masses of all the atoms present in the chemical formula of any compound. One mole of substance contains 6.02×1023 atoms or molecules. This number is known as the Avogadro number.

Answer to Problem 2.43E

The three relationships (equalities) based on the mole concept for given element are,

9.012gBe=1molBe … (1)

1molBe=6.02×1023Beatoms … (2)

6.02×1023Beatoms=9.012gBe … (3)

Explanation of Solution

The molar mass of beryllium is 9.012g/mol. This is the mass of one mole of beryllium. The relationship between the molar mass and moles is shown below.

9.012gBe=1molBe … (1)

The conversion factor corresponding to the given relationship is,

9.012gBe1mol and 1mol9.012gBe

One mole of beryllium contains 6.02×1023 atoms. The relationship between the number of atoms and moles is shown below.

1molBe=6.02×1023Beatoms … (2)

The conversion factor corresponding to the given relationship is,

6.02×1023atoms1mol and 1mol6.02×1023atoms

From the equalities (1) and (2), the mass of 6.02×1023 atoms of beryllium is 9.012g. The relationship between molar mass and number of atoms is shown below.

6.02×1023Beatoms=9.012gBe … (3)

The conversion factor corresponding to the given relationship is,

6.02×1023atoms9.012gBe and 9.012gBe6.02×1023atoms

Conclusion

The three relationships (equalities) based on the mole concept for given element are,

9.012gBe=1molBe …(1)

1molBe=6.02×1023Beatoms…(2)

6.02×1023Beatoms=9.012gBe …(3)

Expert Solution
Check Mark
Interpretation Introduction

(b)

Interpretation:

The three relationships (equalities) based on the mole concept for given element are to be stated.

Concept introduction:

Molar mass is the sum of the atomic masses of all the atoms present in the chemical formula of any compound. One mole of substance contains 6.02×1023 atoms or molecules. This number is known as the Avogadro number.

Answer to Problem 2.43E

The three relationships (equalities) based on the mole concept for given element are,

207.2gPb=1molPb … (1)

1molPb=6.02×1023Pbatoms … (2)

6.02×1023Pbatoms=207.2gPb … (3)

Explanation of Solution

The molar mass of lead is 207.2g/mol. This is the mass of one mole of lead. The relationship between the molar mass and moles is as follows:

207.2gPb=1molPb…(1)

The conversion factor corresponding to the given relationship is,

207.2gPb1mol and 1mol207.2gPb

One mole of lead contains 6.02×1023 atoms. The relationship between the number of atoms and moles is shown below.

1molPb=6.02×1023Pbatoms…(2)

The conversion factor corresponding to the given relationship is,

6.02×1023atoms1mol and 1mol6.02×1023atoms

From the equalities (1) and (2), the mass of 6.02×1023 atoms of lead is 207.2g. The relationship between molar mass and number of atoms is shown below.

6.02×1023Pbatoms=207.2gPb…(3)

The conversion factor corresponding to the given relationship is,

6.02×1023atoms207.2gPb and 207.2gPb6.02×1023atoms

Conclusion

The three relationships (equalities) based on the mole concept for given element are,

207.2gPb=1molPb…(1)

1molPb=6.02×1023Pbatoms…(2)

6.02×1023Pbatoms=207.2gPb…(3)

Expert Solution
Check Mark
Interpretation Introduction

(c)

Interpretation:

The three relationships (equalities) based on the mole concept for given element are to be stated.

Concept introduction:

Molar mass is the sum of the atomic masses of all the atoms present in the chemical formula of any compound. One mole of substance contains 6.02×1023 atoms or molecules. This number is known as the Avogadro number.

Answer to Problem 2.43E

The three relationships (equalities) based on the mole concept for given element are,

23.00gNa=1molNa…(1)

1molNa=6.02×1023Naatoms…(2)

6.02×1023Naatoms=23.00gNa…(3)

Explanation of Solution

The molar mass of sodium is 23.00g/mol. This is the mass of one mole of sodium. The relationship between the molar mass and moles is shown below.

23.00gNa=1molNa…(1)

The conversion factor corresponding to the given relationship is,

23.00gNa1mol and 1mol23.00gNa

One mole of sodium contains 6.02×1023 atoms. The relationship between the number of atoms and moles is shown below.

1molNa=6.02×1023Naatoms…(2)

The conversion factor corresponding to the given relationship is,

6.02×1023atoms1mol and 1mol6.02×1023atoms

From the equalities (1) and (2), the mass of 6.02×1023 atoms of sodium is 23.00g. The relationship between molar mass and number of atoms is shown below.

6.02×1023Naatoms=23.00gNa…(3)

The conversion factor corresponding to the given relationship is,

6.02×1023atoms23.00gNa and 23.00gNa6.02×1023atoms

Conclusion

The three relationships (equalities) based on the mole concept for given element are,

23.00gNa=1molNa…(1)

1molNa=6.02×1023Naatoms…(2)

6.02×1023Naatoms=23.00gNa…(3)

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!
Students have asked these similar questions
Properly write the following formulas: a. Cobalt II Chloride b. Calcium Nitride c. Potassium Phosphite d. Ammonium Ion e. Cadmium Hydroxide
The average atomic mass of carbon is 12.011 amu. Assuming you were able to pick up only one carbon atom, the chance that you would get one with a mass of 12.011 amu is ________. Explain in a few words.
e macroscopic structure level is: A. Structural elements that may be viewed with naked eye B. Electrons within the individual atoms and interactions with their nuclei - C. The organization of atoms or molecules relative to each other o D. Large groups of atoms that normally form together as round mass

Chapter 2 Solutions

Chemistry for Today: General, Organic, and Biochemistry

Ch. 2 - Determine the number of electrons that would have...Ch. 2 - Determine the number of electrons that would have...Ch. 2 - Determine the number of electrons and protons...Ch. 2 - Determine the number of electrons and protons...Ch. 2 - Prob. 2.15ECh. 2 - Prob. 2.16ECh. 2 - Write symbols like those given in Exercises 2.15...Ch. 2 - Write symbols like those given in Exercises 2.15...Ch. 2 - Prob. 2.19ECh. 2 - Prob. 2.20ECh. 2 - Write isotope symbols for neutral atoms with the...Ch. 2 - Write isotope symbols for neutral atoms with the...Ch. 2 - Write the symbols and names for two elements whose...Ch. 2 - Round atomic weights to the nearest whole number,...Ch. 2 - Round atomic weights to the nearest whole number,...Ch. 2 - What are the symbol and name for an element whose...Ch. 2 - In the first 36 elements, 6 elements have atoms...Ch. 2 - What are the symbol and name of the element whose...Ch. 2 - Prob. 2.29ECh. 2 - Prob. 2.30ECh. 2 - The molecular weight was determined for a gas that...Ch. 2 - A flammable gas is known to contain only carbon...Ch. 2 - Glycine, an amino acid found in proteins, has a...Ch. 2 - Serine, an amino acid found in proteins, has a...Ch. 2 - Naturally occurring sodium has a single isotope....Ch. 2 - Naturally occurring aluminum has a single isotope....Ch. 2 - Calculate the atomic weight of lithium on the...Ch. 2 - Calculate the atomic weight of boron on the basis...Ch. 2 - Calculate the atomic weight of silicon on the...Ch. 2 - Calculate the atomic weight of copper on the basis...Ch. 2 - Refer to the periodic table and determine how many...Ch. 2 - Refer to the periodic table and determine how many...Ch. 2 - Write three relationships equalities based on the...Ch. 2 - Write three relationships equalities based on the...Ch. 2 - Use a factor derived from the relationships...Ch. 2 - Use a factor derived from the relationships...Ch. 2 - Prob. 2.47ECh. 2 - Refer to the periodic table and calculate the...Ch. 2 - Prob. 2.49ECh. 2 - Prob. 2.50ECh. 2 - Answer the following questions based on the...Ch. 2 - Answer the following questions based on...Ch. 2 - How many moles of N2O5 contain the same number of...Ch. 2 - How many grams of C2H6O contain the same number of...Ch. 2 - Prob. 2.55ECh. 2 - Determine the mass percentage of hydrogen in CH4...Ch. 2 - Prob. 2.57ECh. 2 - Prob. 2.58ECh. 2 - Urea (CH4N2O) and ammonium sulfate (N2H8SO4) are...Ch. 2 - Prob. 2.60ECh. 2 - Prob. 2.61ECh. 2 - Prob. 2.62ECh. 2 - Prob. 2.63ECh. 2 - The mass of a single carbon 12 atom is 1.991023g....Ch. 2 - Prob. 2.65ECh. 2 - Prob. 2.66ECh. 2 - a. Explain how atoms of different elements differ...Ch. 2 - The atomic weight of aluminum is 26.98u and the...Ch. 2 - Answer the question in the caption of Figure 2.3...Ch. 2 - Answer the question in the caption of Figure 2.5...Ch. 2 - Prob. 2.71ECh. 2 - Prob. 2.72ECh. 2 - Prob. 2.73ECh. 2 - Prob. 2.74ECh. 2 - Prob. 2.75ECh. 2 - Which one of the following substances is a...Ch. 2 - Which of the following is true about compounds?...Ch. 2 - C1734l has a.17 protons, 17 electrons, and 17...Ch. 2 - If two atoms are isotopes, they will a.have same...Ch. 2 - Copper (Cu) has an atomic number of 29 and a mass...Ch. 2 - Atoms are electrically neutral. This means that an...Ch. 2 - The negative charged particle found within the...Ch. 2 - Prob. 2.83ECh. 2 - Prob. 2.84ECh. 2 - The mass of an atom is almost entirely contributed...Ch. 2 - Which of the following is the chemical symbol for...Ch. 2 - Prob. 2.87ECh. 2 - What is the mass number of an atom with 60...Ch. 2 - Which of the following represents Avogadros...Ch. 2 - Which of the following has the greatest number of...Ch. 2 - The formula of carbon dioxide is CO2. Its...Ch. 2 - What is the molar mass of calcium oxide, CaO? a....Ch. 2 - How many grams are contained in 0.200mol of...Ch. 2 - How many moles are contained in a 54.0g sample of...
Knowledge Booster
Background pattern image
Chemistry
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.
Similar questions
SEE MORE QUESTIONS
Recommended textbooks for you
Text book image
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Cengage Learning
Text book image
Introductory Chemistry For Today
Chemistry
ISBN:9781285644561
Author:Seager
Publisher:Cengage
Text book image
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Text book image
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY