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In a periodic table, the average atomic ...

In a periodic table, the average atomic mass of magnesium is given as `24.312 u`. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are `._12Mg^(24) (23.98504u)`, `._(12)Mg^(25) (24.98584)` and `._12Mg^(26) (25.98259 u)`. The natural abundance of `._12Mg^(24)` is `78.99%` by mass. Calculate the abundances of the other two isotopes.

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`""_(12)^(25)Mg:9.3%, ""_(12)^(26)Mg:11.7%`
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In a periodic table, the average mass of magnesium is given as 24.312 u. The average value of based on their relative natural abudance on earth. The three isotopes and their masses are ""_(12)^(24)Mg (23.98504 u), ""_(12)^(25)Mg(24.98584 u) and ""_(42)^(26)Mg(25.98259u) . The natural abundance of ""_(12)^(24)Mg is 78.99% by mass. Calculate the abundances of ther two isotopes.

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