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5 October, 03:18

Antimony has 2 stable isotopes 121-sb mass 120.9038 and 123-sb mass 122.9042 amu. calculate the percent abundances of these isotopes. hint: use amu from periodic table and assign x value as decimal abundance for one isotope and 1-x value for other to solve.

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  1. 5 October, 05:46
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    The atomic mass of an element is a result of the weighted average of the masses of its corresponding isotopes.

    We are given:

    Sb-121: mass of 120.9038 amu, x abundance

    Sb-123: mass of 122.9042 amu, 1-x abundance

    To be able to calculate the atomic mass of antimony, we multiply the percent abundances of the isotopes by their respective atomic masses. Then, we add,

    Atomic mass = (Atomic Mass of Sb-121) (% Abundance) + (Atomic Mass of Sb-123) (% Abundance)

    121.760 amu = (120.9038 amu) (x) + (122.9042 amu) (1 - x)

    Solving for x,

    120.9038x + 122.9042 - 122.9042x = 121.760

    x = 0.57096 or 57.096%

    1-x = 1-0.57096 = 0.42904 or 42.90%
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