number 1 please 11:43Done11 of 11Fe*2562624Cu*12934632927For the next two sections you must show all of your work forcredit.Average Atomic Mass Calculations1. The noble gas, neon, has three isotopes of masses, 22, 21, and 20.If the isotopes have the abundance 8.01%, 1.99% and 90.00%respectively, what is the average atomic mass of neon atoms?2. A naturally occurring same of an element consists of two isotopes,one of mass 85 and one of mass 87. The abundance of theseisotopes is 71% and 29%. Calculate the average atomic mass ofan atom of this element.3. If 6°Ga and 7"Ga occur in the %'s 62.1 and 37.9, calculate theaverage atomic mass of gallium atoms.Percent Abundance1. A sample of Germanium has an average mass of 72.63 amu. If thesample is composed of only Ge-70 and Ge-74, what is the percentabundance of each isotope?2. What is the relative abundance of each isotope present in a sampleof Tin if the average atomic mass of the sample is 118.711 amuand only contains isotopes Sn-118 and Sn-122?

Average atomic mass calculation: (1) Consider the given information is as follows;…

Answered: 1. The noble gas, neon, has three…

1. The noble gas, neon, has three isotopes of masses, 22, 21, and 20. If the isotopes have the abundance 8.01%, 1.99% and 90.00% respectively, what is the average atomic mass of neon atoms?

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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Question

number 1 please

11:43
Done
11 of 11
Fe*2
56
26
24
Cu*1
29
34
63
29
27
For the next two sections you must show all of your work for
credit.
Average Atomic Mass Calculations
1. The noble gas, neon, has three isotopes of masses, 22, 21, and 20.
If the isotopes have the abundance 8.01%, 1.99% and 90.00%
respectively, what is the average atomic mass of neon atoms?
2. A naturally occurring same of an element consists of two isotopes,
one of mass 85 and one of mass 87. The abundance of these
isotopes is 71% and 29%. Calculate the average atomic mass of
an atom of this element.
3. If 6°Ga and 7"Ga occur in the %'s 62.1 and 37.9, calculate the
average atomic mass of gallium atoms.
Percent Abundance
1. A sample of Germanium has an average mass of 72.63 amu. If the
sample is composed of only Ge-70 and Ge-74, what is the percent
abundance of each isotope?
2. What is the relative abundance of each isotope present in a sample
of Tin if the average atomic mass of the sample is 118.711 amu
and only contains isotopes Sn-118 and Sn-122?

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