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21 January, 07:28

What is the atomic weight of a hypothetical element consisting of two isotopes, one with a mass of 62.2 u which is 24% abundant, and the other with a mass of 64.0 u?

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  1. 21 January, 09:21
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    The atomic weight of hypothetical element will be 63.568 amu.

    Explanation:

    Given dа ta:

    First isotope mass = 62.2 amu

    Percentage abundance of first isotope = 24%

    Mass of second isotope = 64 amu

    Percentage abundance of second isotope = 100 - 24 = 76%

    Solution:

    The atomic weight of hypothetical element will be the average atomic mass of its isotopes.

    Average atomic mass = [mass of isotope * its abundance] + [mass of isotope * its abundance] + ... [ ] / 100

    Now we will put the values in formula.

    Average atomic mass = [24 * 62.2] + [76 * 64] / 100

    Average atomic mass = 1492.8 + 4864 / 100

    Average atomic mass = 6356.8/100

    Average atomic mass = 63.568 amu
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