How Do You Calculate Natural Abundance of Isotopes?


The atomic weight of an element is the relative atomic mass of that element. It is the mass weight of the elements, isotopes if any, and their relative abundance.The sum of the percentages of the isotopes is equal to 1 (100%), so the relative abundance of the isotopes can be found using simple algebra. To calculate Natural Abundance of Isotopes, you need to note the atomic mass of an isotope number and the % abundance of each isotope, multiply each of them by their atomic mass and add them together.
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1. Gather the necessary information. You need to know the average atomic mass of the element in question. You will also need to know the atomic mass of each individual isotope for
Since 6.0151 (x) + 7.0160 (1-x) = 6.941. So we get 6.0151x - 7.0160x = 6.941 -7.0160. 1.0009x = 0.075. x = .0749. So the 6.0151 amu has a 7.49 % abundance and the 7.0160 amu has a
If Helium has to naturally occuring isotopes, helium-3 and helium-4. The average atomic mass of helium is 4.003 you. Which isotope
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