Question

The atomic masses of ^{203}Tl and ^{205}Tl are
202.972336 and 204.974410 amu, respectively. The average atomic
mass of thallium is 204.383 amu. Calculate the natural abundances
of these two isotoped.

Percent abundance of ^{203}Tl: ____%

Percent abundance of ^{205}Tl: _____%

Answer #1

Assuming only the above mentioned isotopes exist in nature,,

Let x% be the abundance of
^{203}Tl, then it is obvious that the abundance of
^{205}Tl is 100-x%

The average atomic mass is the sum of individual atomic masses times their corresponding abundance.

Then we have,

202.972336 * x% +204.974410 * (100-x)% = 204.383

- 2.002074 x% + 204.9744410 = 204.383

0.591441/2.002074 = 0.2954

All measured in amu.

by solving for x we get, x = 0.2954 ie
abundance of Li(6) is 29.54% aboundance of ^{203}Tl

70.56 % aboundance of
^{205}Tl

The average atomic mass of nickel is 58.693 amu. Given the data
in the following table, what is the natural abundance of
nickel-64?
58Ni: 57.935 amu 68.0769% abundance
60Ni: 59.931 amu 26.2231% abundance
61Ni: 60.931 amu 1.1399% abundance
62Ni: 61.928 amu 3.6345% abundance
64Ni: 63.928 amu ? % abundance

Chlorine has two naturally occurring isotopes, 35Cl with an
atomic mass of 34.969 amu and 37Cl with an atomic mass of 36.966
amu. The weighted average atomic mass of chlorine is 35.45 amu.
What is the percent abundance of each isotope? Be sure your work
supports your answer.
Copper has two naturally occurring isotopes, 63Cu with an atomic
mass of 62.9296 amu and 65Cu with an atomic mass of 64.9278 amu.
The weighted average atomic mass of copper is 63.546...

A fictional element has two isotopes. Isotope 1 has a mass of
70.0 amu and a relative abundance of 80.28%.
Isotope 2 has a mass of 87.0 amu.
Find the relative abundance (%) of Isotope
Calculate the average atomic mass of the fictional element.

Gallium has two naturally occuring isotopes: Ga-69 with a mass
of 68.9256 amu and a natural abundance of 60.11% and Ga-71. Use the
atomic mass of gallium listed in the periodic table to determine
the mass of Ga-71. How do I figure out this isotopic problem
without the amu of gallium 71. I know how to get the abundance but
not the amu from this slim figures.

Gallium has two naturally occurring isotopes: 69Ga with a mass
of 68.9256 amu and a natural abundance of 60.11% and 71Ga. Use the
atomic mass of gallium from the periodic table to find the mass of
gallium-71. Express the mass in atomic mass units to two
decimal places.

Magnesium has three naturally occurring isotopes: Mg-24 with
mass 24.3050 amu and a natural abundance of 78.99 %, Mg-25 with
mass 24.9858 amu and a natural abundance of 10.00 %, and Mg-26 with
mass 25.9826 amu and a natural abundance of 11.01 %.

Lead (Pb) exists as four naturally occuring isotopes:
204Pb, 206Pb, 207Pb, and
208Pb. Using the data from the table below, calculate
the atomic mass of 208Pb.
Isotope
Atomic Mass (amu)
Natural Abundance (%)
204Pb
203.973
1.4
206Pb
205.974
24.1
207Pb
206.976
22.1
208Pb
?
?
Average Atomic Mass
207.2 amu
100

A) A compound composed of sulfur and fluorine is found to
contain 62.79% by mass of sulfur. If the molar mass of the compound
is 102.13 g/mol, what is its molecular formula?
1-S2F2
2-S2F
3-SF
4-S2F4
5-S3F
show your work (explian)
B)A hypothetical element consists of two isotopes of masses
74.95 amu and 76.95 amu with abundances of 34.9% and 65.1%,
respectively. What is the average atomic mass of this element?
1-76.95 amu
2-74.95 amu
3-75.95 amu
4-75.6 amu
5-76.3...

using average atomic masses for each of the following
elements calculate the mass in any of 5x10"25 sodium atoms

Calculate the quantity of energy produced per mole of U-235
(atomic mass = 235.043922 amu) for the neutron-induced fission of
U-235 to produce Te-137 (atomic mass = 136.9253 amu) and Zr-97
(atomic mass = 96.910950 amu).

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