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An element exists as only three stable isotopes. rnrnisotope 1 has a mass of 573.5 amu and an abundance of 38.5%. Isotope 2 has a mass of 579.4 amu and an abundance of 45.0%. Isotope 3 has a mass of 582.3 amu and an abundance of 16.5%. What is the weighted average atomic weight of this element?
Accepted Answer
The weighted average atomic weight of this element can be calculated as follows:
Weighted Average Atomic Weight = (Mass of Isotope 1 × Abundance of Isotope 1) + (Mass of Isotope 2 × Abundance of Isotope 2) + (Mass of Isotope 3 × Abundance of Isotope 3)
= (573.5 amu × 0.385) + (579.4 amu × 0.450) + (582.3 amu × 0.165)
= 220.4 amu + 260.7 amu + 96.0 amu
= 577.1 amu
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