Element Y has two natural isotopes Y-63 (62.940 amu) and Y-65 (64.928 amu). Calculate the atomic mass of element Y, given the abundance of Y-63 is 69.17%?

Question

Chemistry

Hailee Delgado

1 November, 21:37

Element Y has two natural isotopes Y-63 (62.940 amu) and Y-65 (64.928 amu). Calculate the atomic mass of element Y, given the abundance of Y-63 is 69.17%?

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Answers (1)

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Pockets · Answer 1

Average atomic mass = 63.553 amu.

Explanation:

Given dа ta:

Abundance of Y-63 = 69.17%

Abundance of Y-65 = 100 - 69.17 = 30.83%

Atomic mass of Y-63 = 62.940 amu

Atomic mass of Y-65 = 64.928 amu

Atomic mass of Y = ?

Solution:

Average atomic mass = (abundance of 1st isotope * its atomic mass) + (abundance of 2nd isotope * its atomic mass) / 100

Average atomic mass = (62.940*69.17) + (64.928*30.83) / 100

Average atomic mass = 4353.560 + 2001.730 / 100

Average atomic mass = 6355.29 / 100

Average atomic mass = 63.553 amu.