Answer:
The atomic weight of hypothetical element will be 63.568 amu.
Explanation:
Given data:
First isotope mass = 62.2 amu
Percentage abundance of first isotope = 24%
Mass of second isotope = 64 amu
Percentage abundance of second isotope = 100- 24 = 76%
Solution:
The atomic weight of hypothetical element will be the average atomic mass of its isotopes.
Average atomic mass = [mass of isotope× its abundance] + [mass of isotope× its abundance] +...[ ] / 100
Now we will put the values in formula.
Average atomic mass = [24 ×62.2] + [76× 64] / 100
Average atomic mass = 1492.8 + 4864 / 100
Average atomic mass = 6356.8/100
Average atomic mass = 63.568 amu
