Iron exists in nature as a mixture of predominantly three isotopes: ⁵⁴₂₆Fe (53.94 amu), ⁵⁶₂₆Fe (55.93 amu), and ⁵⁷₂₆Fe (56.94 amu). If the most common isotope, ⁵⁶₂₆Fe, accounts for 91.75% of iron atoms, and the average atomic mass of iron is 55.85 amu, what is the percent abundance of the rarest of these three isotopes of iron?
Iron exists in nature as a mixture of predominantly three isotopes: ⁵⁴₂₆Fe (53.94 amu), ⁵⁶₂₆Fe (55.93 amu), and ⁵⁷₂₆Fe (56.94 amu). If the most common isotope, ⁵⁶₂₆Fe, accounts for 91.75% of iron atoms, and the average atomic mass of iron is 55.85 amu, what is the percent abundance of the rarest of these three isotopes of iron?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter3: Mass Relations In Chemistry; Stoichiometry
Section: Chapter Questions
Problem 31QAP: Combustion analysis of 1.00 g of the male sex hormone, testosterone, yields 2.90 g of CO2 and 0.875...
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Iron exists in nature as a mixture of predominantly three isotopes: ⁵⁴₂₆Fe (53.94 amu), ⁵⁶₂₆Fe (55.93 amu), and ⁵⁷₂₆Fe (56.94 amu). If the most common isotope, ⁵⁶₂₆Fe, accounts for 91.75% of iron atoms, and the
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How did you know to make Fe 54 x and Fe 57 .0825 -x
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