A naturally occurring sample of an element contains only two isotopes. The first isotope has a mass of 62.9296 amu and a natural abundance of 69.15 %. The second isotope has a mass of 64.9278 amu. You may want to reference (Page) Section 2.8 while completing this problem Part A Find the atomic mass of the element. 64.58 amu O 63.55 amu O 69.72 amu O 63.05 amu Submit Request Answer

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16-12-2022
Chemistry

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A naturally occurring sample of an element contains only two isotopes. The first isotope has a mass of 62.9296 amu and a natural abundance of 69.15 %. The second isotope has a mass of 64.9278 amu. You may want to reference (Page) Section 2.8 while completing this problem Part A Find the atomic mass of the element. 64.58 amu O 63.55 amu O 69.72 amu O 63.05 amu Submit Request Answer

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durbansa43 durbansa43 · Answer 1 · 2022-12-20T10:21:13-05:00

correct answer is 63.22 amu.

Determining the atomic mass of an element requires calculating the weighted average of the masses of the two isotopes, taking into account their natural abundance. The atomic mass of an element is given by the formula:

Atomic mass = (mass of isotope 1 × natural abundance of isotope 1) + (mass of isotope 2 × natural abundance of isotope 2)

Inserting the values given in the question gives:

Atomic mass = (62.9296 amu × 0.6915) + (64.9278 amu × (1 - 0.6915))

= 43.40 amu + 19.82 amu

= 63.22 am

Therefore, the atomic mass of the element is 63.22 amu.

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