Calculations Using the Mole Learning Goal: 2.32x1023 13C atoms To learn how to convert grams to moles and to use the mole to find the number of atoms in a sample. Submit Previous Answers The mole (abbreviated mol) is a counting unit used to simplify calculations that would otherwise involve very large numbers. The mole is equivalent to the number of carbon atoms in exactly 12 g of isotopically pure 6.02 x 1023. This number is known as Avogadro's number in honor of Amedeo Avogadro. 12 C, or v Correct Avogadro's number can be used as a conversion factor between moles and atoms as shown here: Part C 6.02x1023 atoms Based on your answer in Part B, how many electrons are in this amount of 13 C? 1 mole of atoms Express your answer numerically in electrons. The molar mass of a substance is the mass of one mole • View Available Hint(s) of a substance and is written in units of grams per mole. The molar mass of an atom is equivalent to its atomic mass whereas the molar mass of a substance is equivalent to its formula weight. x" |X| x•10" electrons
Calculations Using the Mole Learning Goal: 2.32x1023 13C atoms To learn how to convert grams to moles and to use the mole to find the number of atoms in a sample. Submit Previous Answers The mole (abbreviated mol) is a counting unit used to simplify calculations that would otherwise involve very large numbers. The mole is equivalent to the number of carbon atoms in exactly 12 g of isotopically pure 6.02 x 1023. This number is known as Avogadro's number in honor of Amedeo Avogadro. 12 C, or v Correct Avogadro's number can be used as a conversion factor between moles and atoms as shown here: Part C 6.02x1023 atoms Based on your answer in Part B, how many electrons are in this amount of 13 C? 1 mole of atoms Express your answer numerically in electrons. The molar mass of a substance is the mass of one mole • View Available Hint(s) of a substance and is written in units of grams per mole. The molar mass of an atom is equivalent to its atomic mass whereas the molar mass of a substance is equivalent to its formula weight. x" |X| x•10" electrons
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
Concept explainers
Atomic Structure
The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.
Shape of the D Orbital
Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.
Question
100%
Part C: Based on your answer in Part B, how many electrons are in this amount of 13C?
Express your answer numerically in electrons.
Part D: Based on your answer in Part B, how many neutrons are in this amount of 13C?
Express your answer numerically in neutrons.
Transcribed Image Text:Calculations Using the Mole
Learning Goal:
13
2.32x1023 C atoms
To learn how to convert grams to moles and to use the
mole to find the number of atoms in a sample.
Submit
Previous Answers
The mole (abbreviated mol) is a counting unit used to
simplify calculations that would otherwise involve very
large numbers. The mole is equivalent to the number of
carbon atoms in exactly 12 g of isotopically pure 12C, or
6.02 × 1023. This number is known as Avogadro's
number in honor of Amedeo Avogadro.
Correct
Avogadro's number can be used as a conversion factor
between moles and atoms as shown here:
Part C
6.02×1023 atoms
Based on your answer in Part B, how many electrons are in this amount of 13C?
1 mole of atoms
Express your answer numerically in electrons.
The molar mass of a substance is the mass of one mole
of a substance and is written in units of grams per mole.
The molar mass of an atom is equivalent to its atomic
mass whereas the molar mass of a substance is
• View Available Hint(s)
equivalent to its formula weight.
ΑΣφ.
?
a
|X|
X•10"
electrons
圓
Expert Solution
Step 1
Trending now
This is a popular solution!
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