Please help thank you! 33.967Activity 3: Atomic MassThe actual mass of a proton or a neutron is verysmall, 1.67x102ªg. The mass of an electron is9.11x10 28g, which is negligible in comparison.Given these values, the mass of even the largestatom is incredibly small.In general, these values are inconveniently smalland impractical to work with. Instead, it is moreuseful to compare the relative masses of atomsusing a reference isotope as a standard. AtomicMasses of elements are calculated Using theabundance of the isotope and its mass in theAtomic Mass Unit (amu).Using the data table above, which gives theatomic mass of an element and is calculatedusing the percent abundance and mass of itsisotopes, answer the following questions.Natural Percent Abundance ofStable Isotopes of Some ElementsNatural percentabundanceNameMass lamu) Atomic mass99.9851.00782.0141HydrogenIH0.0151.0079negligible3.0160HeHe0.000199.99993.01604.0026Helium4.002698.89Carbon12.00013.00312.011L11IN99.63Nitrogen14.00315.00014.007IN0.3799.7590 0370.20415.99516.99517999Окудеn15.99910US95.0020.764.220.01431.97232.97133.96735.967Sulfur32.06ICI75.7724.2334.969Chlorine35.45336 9661. Whichisotopeoxygen (0) istheabundant?ofmostWhat is itspercentabundance?2. How couldyou use theatomic massof helium todeterminewhich isotopeof helium ismostabundant?3. Whichisotopesulfur (S) isoftheleastabundant?What is itspercentabundance?

1) O816 is the most abundant isotope of oxygen according to the given data with a 99.7599…

1. Which of isotope oxygen (0) is the most abundant? What is its percent abundance? 2. How could you use the atomic mass of helium to determine which isotope of helium is most abundant? 3. Which of isotope sulfur (S) is least the abundant? What is its percent abundance?

1. Which of isotope oxygen (0) is the most abundant? What is its percent abundance? 2. How could you use the atomic mass of helium to determine which isotope of helium is most abundant? 3. Which of isotope sulfur (S) is least the abundant? What is its percent abundance?

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...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

Please help thank you!

33.967
Activity 3: Atomic Mass
The actual mass of a proton or a neutron is very
small, 1.67x102ªg. The mass of an electron is
9.11x10 28g, which is negligible in comparison.
Given these values, the mass of even the largest
atom is incredibly small.
In general, these values are inconveniently small
and impractical to work with. Instead, it is more
useful to compare the relative masses of atoms
using a reference isotope as a standard. Atomic
Masses of elements are calculated Using the
abundance of the isotope and its mass in the
Atomic Mass Unit (amu).
Using the data table above, which gives the
atomic mass of an element and is calculated
using the percent abundance and mass of its
isotopes, answer the following questions.
Natural Percent Abundance of
Stable Isotopes of Some Elements
Natural percent
abundance
Name
Mass lamu) Atomic mass
99.985
1.0078
2.0141
Hydrogen
IH
0.015
1.0079
negligible
3.0160
He
He
0.0001
99.9999
3.0160
4.0026
Helium
4.0026
98.89
Carbon
12.000
13.003
12.011
L11
IN
99.63
Nitrogen
14.003
15.000
14.007
IN
0.37
99.759
0 037
0.204
15.995
16.995
17999
Окудеn
15.999
10
US
95.002
0.76
4.22
0.014
31.972
32.971
33.967
35.967
Sulfur
32.06
ICI
75.77
24.23
34.969
Chlorine
35.453
36 966
1. Which
isotope
oxygen (0) is
the
abundant?
of
most
What is its
percent
abundance?
2. How could
you use the
atomic mass
of helium to
determine
which isotope
of helium is
most
abundant?
3. Which
isotope
sulfur (S) is
of
the
least
abundant?
What is its
percent
abundance?

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