In nature, the element X consists of two naturally occurring isotopes. 107X with abundance 55.84% and isotopic mass 106.9051 amu and 109X with isotopic mass 108.9048 amu. Use the given information to calculate the atomic mass of the element X to an accuracy of .001% (Report your answer like this yyy.yyyy)
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Expert's answer
2015-09-13T04:19:33-0400
«W» is the mass fraction (abundance) of the isotope (%); W(107X) = 55.84%; W(109X) = 100 – 55.84 = 44.16%; Ar – the relative atomic mass (a.m.u.) of the element. Symbol: u; Ar107X = 106.9051 amu (u); Ar109X = 108.9048 amu (u); ArX=W(107X)*Ar107X+W(109X)*Ar109X ArX = 106.9051*0.5584 + 108.9048*0.4416 = 59.6958 + 48.0924 = 107.7882 amu (u); Answer: 107.7882
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