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3 November, 19:01

Magnesium has three naturally occurring isotopes with masses of 23.99 amu, 24.99 amu, and 25.98 amu and natural abundances of 78.99%, 10.00%, and 11.01%, respectively. Calculate the atomic mass of magnesium

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  1. 3 November, 19:19
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    Answer: 24.309

    Explanation:

    Isotope A:

    Mass number = 23.99 amu

    Abundance = 78.99%

    Isotope B:

    Mass number = 24.99 amu

    Abundance = 10.00%

    Isotope C:

    Mass number = 25.98 amu

    Abundance = 11.01%

    To find the atomic Mass of magnesium, we must add the product of the mass number and abundance of each of the isotopes. In doing so, we have:

    Let M1 and A be the mass number and the abundance for isotope A.

    Let M2 and B be the mass number and the abundance of isotope B

    Let M3 and C be the mass and abundance of isotopeC

    Atomic mass = (M1 x A) + (M2 x B) + (M3 x C)

    = (23.99x78.99%) + (24.99x10%) + (25.98x11.01%)

    = 18.950 + 2.499 + 2.860

    = 24.309

    The atomic mass of magnesium is 24.309
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