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SOLVED: Calculate the average atomic mass of iron using the isotopes in Table 2 below: Table 2. Stable Isotopes of Iron Isotope Mass (amu) % Abundance 54Fe 53.94 5.845 56Fe 55.93 91.75 57Fe 56.94 2.119
![CHEMISTRY; I'm not quite sure what I'm doing. [University Chemistry:Elements] what is the percent abundance of the rarest of these three isotopes of iron? : r/HomeworkHelp](https://preview.redd.it/1mzcw4zdk4291.jpg?width=640&crop=smart&auto=webp&s=c33f44ee48508606efd795243fde7444e5a854d6 "CHEMISTRY; I'm not quite sure what I'm doing. [University Chemistry:Elements] what is the percent abundance of the rarest of these three isotopes of iron? : r/HomeworkHelp")
CHEMISTRY; I'm not quite sure what I'm doing. [University Chemistry:Elements] what is the percent abundance of the rarest of these three isotopes of iron? : r/HomeworkHelp
54Fe Isotope, Enriched 54Fe, 54Fe Metal, 54Fe Oxide, 54Fe Price
Naturally occurring iron consists of four isotopes with the abundances indicated here. From the masses and relative abundances of these isotopes, calculate the atomic weight of naturally occurring iron. | Homework.Study.com
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iron 57 – AMT Stable Isotopes
Given that the abundances of isotopes ^54Fe, ^56Fe and ^57Fe are 5%, 90% and 5% respectively, the atomic mass of Fe is:
Given that the abundances of isotopes ^54Fe, ^56Fe and ^57Fe are 5%, 90% and 5% respectively, the atomic mass of Fe is:
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