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19 January, 21:23

Indium has only two naturally occurring isotopes. the mass of indium-113 is 112.9041 amu and the mass of indium-115 is 114.9039 amu. part a use the atomic mass of indium to calculate the relative abundance of indium-113.

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  1. 19 January, 21:26
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    The average atomic mass written in the periodic table is determined from the relative abundances of the element's isotopes. The equation would be:

    Average Atomic Mass = ∑ (Relative Abundance*Mass)

    Let be the relative abundance of Indium-113. Because there are only 2 isotopes, their relative abundances should equal to 1, such that the relative abundance for Indium-15 is (1-x). The atomic mass of indium is 114.818 amu.

    x (112.9041) + (1 - x) (114.9039) = 114.818

    Solving for x,

    x = 0.043 or 4.3%
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