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22 June, 19:10

A certain element consists of two stable isotopes. the first has a mass of 68.9 amu and a percent natural abundance of 60.4 %. the second has a mass of 70.9 amu and a percent natural abundance of 39.6 %. what is the atomic weight of the element?

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  1. 22 June, 21:58
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    The average atomic weight of this element can be calculated as follows:

    average atomic weight =

    (atomic weight of first isotope) (its percentage of abundance) +

    (atomic weight of second isotope) (its percentage of abundance)

    atomic weight of first isotope = 68.9 amu

    its percentage of abundance = 0.604

    atomic weight of second isotope = 70.9 amu

    its percentage of abundance = 0.396

    So, just substitute in the above equation to get the atomic weight of the element as follows:

    atomic weight = (68.9) (0.604) + (70.9) (0.396) = 69.692 amu
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