Silver has an atomic mass of 107.868 amu. the ag-109 isotope (108.91 amu) is 48.16%. what is the mass, in amu, of the other isotope? 105.87 amu 106.12 amu 106.91 amu 108.47 amu

The mass, in amu, of the other isotope of the silver is 106.91 amu

Let the 1st isotope be A

Let the 2nd isotope be B

From the question given above, the following data were obtained:

Atomic mass of Ag = 107.868 amu

Mass of A = 108.91 amu

Abundance of A (A%) = 48.16%

Abundance of B (B%) = 100 – 48.16 = 51.84%

The mass of the other isotope can be obtained as follow:

Atomic mass = [(mass of A × A%)/100] + [(mass of B × B%)/100]

107.868 = [(108.91 × 48.16)/100] + [(mass of B × 51.84)/100]

107.868 = 52.451056 + mass of B × 0.5184

Collect like terms

107.868 – 52.451056 = mass of B × 0.5184

55.416944 = mass of B × 0.5184

Divide both side by 0.5184

Mass of B = 55.416944 / 0.5184

Therefore, the mass of the other isotope is 106.91 amu

Learn more: link

Option C: 106.91 amu

Atomic mass of silver is 107.868 amu. Mass of Ag-109 isotope is 108.91 amu and its percentage abundance is 48.16%, let the mass of other isotope be X, the percentage abundance can be calculated as:

%X=100-48.16=51.84%

Atomic mass of an element  is calculated by taking sum of atomic masses of its isotopes multiplied by their percentage abundance.

Thus,

Atomic mass= m(Ag-109)×%(Ag-109)+X×%(Ag-X)

Putting the values,

Thus,

Therefore, other isotope is Ag-106.9, which is close to option C.

organisms are more likely to be more preserved in mud than sand because mud is moist and wet, while sand is very dry.