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1 May, 16:51

Suppose that a fictitious element, X, has two isotopes: 59X (59.015 amu) and 62X (62.011 amu). The lighter isotope has an abundance of 81.7%. Calculate the atomic mass of the element X.

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  1. 1 May, 20:29
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    Atomic Mass of Element = 59.57 amu

    Given dа ta:

    Element X Isotope 1 atomic weight = 59.015 amu

    Element X Isotope 2 atomic weight = 62.011 amu

    The abundance of lighter isotope = 81.7%

    Atomic Mass of Element X = ?

    Solution:

    81.7% is the abundance of element that is lighter so it is the of the isotope having weight 59.015 amu

    Then the remaining abundance = 100 - 81.7 = 18.3 %

    18.3 % abundance of the isotope weight = 62.011 amu

    Formula:

    Mass of the element = % of abundance (atomic mass of Isotope 1) + % of abundance (atomic mass of Isotope 2)

    Put the values

    Atomic mass of Element X = 81.7/100 (59.015) + 18.3 / 100 (62.011)

    Atomic mass of Element = 0.817 (59.015) + 0.183 (62.011)

    Atomic mass of Element = 48.22 + 11.35

    Atomic Mass of Element = 59.57 amu
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