What is the atomic weight of a hypothetical element consisting of two isotopes, one with a mass of 62.2 u which is 24% abundant, and the other with a mass of 64.0 u?

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

tracks, burrows, eggshells, nests, tooth marks, or gastroliths

in the analysis of systems that involve fluid flow, we frequently encounter the combination of properties u and pv.