Answer:
To determine the identity and atomic mass of the other isotope of silver (Ag), we can use the given information about the percentage abundance and atomic mass of Ag-107.
Let's assume that the other isotope is Ag-x, where x represents the mass number of the isotope. Since the total percentage abundance of both isotopes must add up to 100%, we can calculate the percentage abundance of Ag-x by subtracting the given percentage abundance of Ag-107 from 100%.
Percentage abundance of Ag-x = 100% - 51.84% = 48.16%
Now, we can set up an equation to find the atomic mass of Ag-x. The equation is as follows:
(percentage abundance of Ag-x / 100) * (atomic mass of Ag-x) + (percentage abundance of Ag-107 / 100) * (atomic mass of Ag-107) = atomic mass of silver
Plugging in the known values:
(48.16 / 100) * (atomic mass of Ag-x) + (51.84 / 100) * (106.9051 amu) = 107.9 amu
Simplifying the equation:
0.4816 * (atomic mass of Ag-x) + 0.5184 * (106.9051 amu) = 107.9 amu
0.4816 * (atomic mass of Ag-x) = 107.9 amu - (0.5184 * 106.9051 amu)
0.4816 * (atomic mass of Ag-x) = 107.9 amu - 55.4072 amu
0.4816 * (atomic mass of Ag-x) = 52.4928 amu
Dividing both sides by 0.4816:
(atomic mass of Ag-x) = 52.4928 amu / 0.4816
(atomic mass of Ag-x) ≈ 108.8 amu
Therefore, the other isotope of silver (Ag-x) has an atomic mass of approximately 108.8 amu.
Step-by-step explanation: