Question

In nature, the element X consists of two naturally occurring isotopes. 107X with abundance 53.84% and isotopic mass 106.9051 amu and 109X with isotopic mass 108.9048 amu. Use the given information to calculate the atomic mass of the element X to an accuracy of .001% (Report your answer like this yyy.yyyy)

Answer 1

Answer:

107.828 amu

Explanation:

Firstly, we need to know the percentage abundance of the second isotope. Since there are 2 naturally occurring isotopes, the percentage abundance of the second isotope will be 100 - 53.84 = 46.16%

Now we go on to deduce the isotopic mass. We do this by multiplying the percentage compositions by the masses.

53.84/100 * 106.9051 = 57.558 amu

46.16/100 * 108.9048 = 50.270 amu

The atomic mass is thus 57.558 + 50.270 = 107.828 amu