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20 September, 19:49

A certain element x has four isotopes. 0.5600% of x has a mass of 83.91343 amu. 9.860% of x has a mass of 85.90927 amu. 7.000% of x has a mass of 86.90890 amu. 82.58% of x has a mass of 87.90562 amu. What is the average atomic mass of element x?

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Answers (2)
  1. 20 September, 20:04
    0
    solution:

    Find the average of atomic weight is

    (0.0056 x 83.91343) + (0.098860 x 85.90927) + (0.07x86.90890) + (0.8258x87.90562) = 87.61665 amu
  2. 20 September, 20:12
    0
    Average Atomic Weight (X) = 87.638974 amu

    Explanation:

    To find the average atomic weight of an unknown element that exhibit multiple isotopes is given by:

    Average Atomic Weight = Percentage of given isotope in the mass spectrum x The corresponding atomic weight of given isotope

    Average Atomic Weight (X) = [0.0056 x 83.91343] + [0.098860 x 85.90927] + [0.07 x 86.90890] + [0.8258 x 87.90562] = 87.638974 amu
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