Question

Naturally occuring element X exists in three isotopic forms: X-28 (27.730 amu, 60.58% abundance), X-29 (28.841 amu, 18.35% abundance), and X-32 (31.321 amu, 21.07% abundance). Calculate the average atomic weight of X. Please enter your answer to 4 significant figures.

Answer 1

The Average atomic weight of X is 28.7amu

Isotopes are atoms with the same number of protons but differing numbers of neutrons.

Different isotopes have various atomic masses.

The proportion of atoms with a particular atomic mass that can be found in a naturally occurring sample of an element is known as the relative abundance of an isotope.

An element's average atomic mass is computed as a weighted average by multiplying the relative abundances of its isotopes by their respective atomic masses, then adding the resulting products.

Using mass spectrometry, it is possible to determine the relative abundance of each isotope.

The atomic weight of the element will be a weighted average of the isotopes based on the relative abundance:

(27.730 x 0.6058) + (28.841 x 0.1835) + (31.321 x 0.2107) = 16.7988 + 5.2923+ 6.599 = 28.690 = 28.7 amu.

Average atomic weight of X is 28.7amu

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