Question

A naturally occurring element consists of three isotopes. The data for the isotopes are:
isotope 1: 46.972 u, 69.472%
isotope 2: 48.961 u, 21.667%
isotope 3: 49.954 u, 8.8610%
What is the average atomic mass of this naturally occurring element?

**** I keep getting an answer that is not one of the multiple choices ****

Answer 1

(46.972* 69.472% + 48.961*21.667% + 49.954*8.8610%)/100% =

= 46.972* 0.69472 + 48.961*0.21667 + 49.954*0.088610 =47.667 u

Answer 2

The atomic mass of the element has been found to be 87.5048 amu.

The atomic mass of the element has been given as the average atomic mass of the atom with respect to the isotopes in the nature and abundance.

The average atomic mass of a compound has been given by:

$\rm amu=mass_1\;\times\;abundance\;+\;mass_2\;\times\;abundance$

Computation for atomic mass

The mass of isotopes of a given element has been given as:

Isotope 1 = 46.972, abundance = 0.69472

Isotope 2= 48.961 abundance = 0.21667

Isotope 3= 49.954 abundance = 0.88610

Substituting the values for atomic mass:

$amu=46.972\;\times\;069472\;+\;48.961\;\times\;0.21667\;+\;49.954\;\times\;0.88610\\amu=32.6323\;+\;10.6083\;+\;44.2642\\amu=87.5048$

The atomic mass of the element has been found to be 87.5048 amu.

For more information about atomic mass., refer to the link:

https://brainly.com/question/5566317