What is the average atomic mass of the isotopes shown in the table? Isotope Abundance (%) Mass of Isotope (amu)
Isotope-A
54.0
17.984
Isotope-B
32.0
18.985
Isotope-C
14.0
19.982

18.58

Explanation:

From the question given above, the following data were:

Isotope A:

Abundance of A = 54%

Mass of A = 17.984 amu

Isotope B:

Abundance of B = 32%

Mass of B = 18.985 amu

Isotope C:

Abundance of C = 14%

Mass of C = 19.982 amu

Average atomic mass =?

AVERAGE = [(Mass of A × A%)/100)] + [(Mass of B × B%)/100] + [(Mass of C × C%)/100]

AVERAGE = [(17.984 × 54%)/100] + [(18.985 × 32%)/100] + [(19.982 × 14%)/100]

= 9.71136 + 6.0752 + 2.79748

= 18.58

Therefore, the average atomic mass of the isotope is 18.58 amu

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qualitative observation deals with data that can be observed with our senses: sight, smell, touch, taste, and hearing. they do not involve measurements or numbers. for instance, colors, shapes, and textures of objects are all qualitative observations.