A hypothetical element consists of four isotopes. Use the information below to calculate the average atomic volume mass of the element. Work must be shown for credits to be given.

104.969 amu.

Explanation:

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

Isotope A:

Mass of A = 107.977 amu

Abundance (A%) = 0.1620%

Isotope B:

Mass of B = 106.976 amu

Abundance (B%) = 1.568%

Isotope C:

Mass of C = 105.974 amu

Abundance (C%) = 47.14%

Isotope D:

Mass of D = 103.973 amu

Abundance (D%) = 51.13%

Average atomic mass =?

The average atomic mass of the element can be obtained as follow:

Average atomic mass = [(Mass of A × A%) /100] + [(Mass of B × B%) /100] + [(Mass of C × C%) /100] + [(Mass of D × D%) /100]

Average atomic mass = [(107.977 × 0.1620)/100] + [(106.976 × 1.568)/100] + [(105.974 × 47.14)/100] + [(103.973 × 51.13)/100]

= 0.175 + 1.677 + 49.956 + 53.161

= 104.969 amu

Therefore, the average atomic mass of the element is 104.969 amu.

it should be p1 v1 = p2 v2