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madreJ [45]
3 years ago
9

Silver has two naturally isotopes and has an atomic mass of 107.868 amu. One isotope is Ag-109 isotope (108.905 amu) and has a n

atural abundance of 48.16%. What is the mass in amu of the other isotope
Chemistry
1 answer:
Triss [41]3 years ago
5 0

Answer:  106.905

Explanation:  If there are only 2 isotopes, and 1 of them is 48.16%, the second must, by default, be (100 - 48.16%) = 51.84%  The final, averaged, atomic mass is 107.868.  This is made up of each isotope's atomic mass times the percentage of that isotope in the total sample.  The weighted value of the known isotope (109) plus that of the unknown must come to the observed value of 107.868 amu.  (107.868 - 52.45 = 55.42).  Divide that by the % for that isotope (55.42/0.5184) = 106.90 amu for the second isotope.

<u>Atomic Mass</u>  <u>% of Sample</u> <u>Weighted Value</u>

    108.905         48.16%              52.45

          X               51.84%              <u>55.42</u>

                                                     107.87

      X = (55.42/0.5184) = 106.90 amu

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