Average atomic mass = ($\text{Mass of isotope 1} \times \text{Fractional abundance of isotope 1}$) + ($\text{Mass of isotope 2} \times \text{Fractional abundance of isotope 2}$) Average atomic mass = $(35 \text{ u} \times 3/4) + (37 \text{ u} \times 1/4)$ Average atomic mass = $(105/4) \text{ u} + (37/4) \text{ u}$ Average atomic mass = $(105 + 37)/4 \text{ u}$ Average atomic mass = $142/4 \text{ u}$ Average atomic mass = $35.5 \text{ u}$.
Chlorine occurs in nature in two isotopic forms of masses 35 u and 37 u in the ratio of 3 : 1 respectively. What is the average atomic mass of the Chlorine atom ?
Asked in UPSC NDA 2 2021 · Topic: Atomic Structure (Isotopes, Isobars, and Isotones)
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