The element with 2 isotopes, one representing 60.4 % of the atoms (68.9257 amu) and the other representing the rest (70.9249 amu), has an atomic mass of 69.7 amu. The element is Gallium.
An element has 2 isotopes. The sum of their abundances is 100%. If the abundance of isotope 1 is 60.4%, the abundance of isotope 2 is:
[tex]ab_1 + ab_2 = 100 \% \\ab_2 = 100\% - ab_1 = 100 \% - 60.4 \% = 39.6 \%[/tex]
Isotope 1 has an abundance of 60.4% and a mass of 68.9257 amu, while Isotope 2 has an abundance of 39.6% and a mass of 70.9249 amu. The atomic mass is the weighted average of the mass by the abundance.
[tex]am = \frac{68.9257 amu \times 60.4 + 70.9249 amu \times 39.6 }{100} = 69.7 amu[/tex]
The element with this atomic mass is Gallium.
The element with 2 isotopes, one representing 60.4 % of the atoms (68.9257 amu) and the other representing the rest (70.9249 amu), has an atomic mass of 69.7 amu. The element is Gallium.
You can learn more about isotopes here: https://brainly.com/question/21536220
