Problem: Naturally occurring magnesium has the following isotopic abundances:IsotopeAbundance Atomic mass (amu) 24 Mg78.99%23.9850425 Mg10.00%24.9858426 Mg11.01%25.98259What is the average atomic mass of Mg?

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atomic mass = [mass×f.a.]isotope 1 + [mass×f.a.]isotope 3 + [mass×f.a.]isotope 2

24 Mg: mass = 23.98504 amu      f.a. = 78.99% ÷ 100 = 0.7899

 25 Mg: mass = 24.98584 amu     f.a. = 10.00% ÷ 100 = 0.1000

26 Mg: mass = 25.98259 amu      f.a. = 11.01% ÷ 100 = 0.1101


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Problem Details
Naturally occurring magnesium has the following isotopic abundances:


IsotopeAbundance Atomic mass (amu
24 Mg78.99%23.98504
25 Mg10.00%24.98584
26 Mg11.01%25.98259


What is the average atomic mass of Mg?

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