The element silver (Ag) has two naturally occuring isotopes:
Ag-107 with a mass of 106.905 amu and
Ag-109
Silver consists of 51.82% Ag-107 and has an average atomic mass of 107.868 amu.
Calculate the mass of Ag-109
plzzzz
2007-11-12 10:50:24 · 3 answers · asked by Sina 2 in Science & Mathematics ➔ Chemistry
We know that Ag-107 has a mass of 107.868 amu and occurs 51.82% in nature. Therefore, Ag-109 occurs 48.18%. We also know that the average amu is 106.905.
We can do the algebra.
(.5182 (the percent) * (107.868amu (Ag-107)) + (.4818 (percent Ag-109) * X (we are solving for the mass Ag-109)) = 106.905 amu (the average)
When we solve for X (the mass Ag-109) we come up with 105.869 amu.
Hope this helps!
2007-11-12 11:02:14 · answer #1 · answered by Anonymous · 0⤊ 0⤋
The reasoning is exactly the same as with the Eu question.
0.5182 x exact mass of 107Ag + (1 - 0.5182) x exact mass of 109Ag = average atomic mass of Ag
2007-11-12 11:01:23 · answer #2 · answered by Facts Matter 7 · 0⤊ 0⤋
Amu Of Silver
2017-02-22 03:22:54 · answer #3 · answered by Anonymous · 0⤊ 0⤋