Question
Asked Sep 14, 2019

Copper has two naturally occurring isotopes, 63Cu (isotopic mass 62.9396 amu) and 65Cu (isotopic mass 64.9278 amu). If copper has an atomic mass of 63.546 amu, what is the percent abundance of 65Cu?

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Expert Answer

Step 1

Given,

Mass of 63Cu (isotope I) = 62.9396 amu

Mass of 65Cu (isotope II) = 64.9278 amu

Atomic mass of Cu (average mass) = 63.546 amu

Let ‘A’ be the abundance of 63Cu (isotope I) then, (1-A) will be the abundance of 65Cu (isotope II).

 

The average mass of Cu is expressed as:

Average mass (Abundance of isotope I x Mass of isotope I
(Abundance of isotope II x Mass of isotope II)
Average mass
[Ax 62.9396 ] + [(1-A) x 64.9278]
=
63.546 62.9396 A + 64.9278 - 64.9278 A
63.546 64.9278
62.9396 A - 64.9278 A
- 1.3818 -1.9882 A
- 1.3818
A =
- 1.9882
0.6950
. (1-A) 1- 0.6950 0.305
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Average mass (Abundance of isotope I x Mass of isotope I (Abundance of isotope II x Mass of isotope II) Average mass [Ax 62.9396 ] + [(1-A) x 64.9278] = 63.546 62.9396 A + 64.9278 - 64.9278 A 63.546 64.9278 62.9396 A - 64.9278 A - 1.3818 -1.9882 A - 1.3818 A = - 1.9882 0.6950 . (1-A) 1- 0.6950 0.305

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Step 2

The percent abundance of the Cu isotopes will be:

      A =...

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