Question

The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. Calculate the average atomic mass of the element in amu. PLEASE HELP ASAP THANK YOU SO MUCH

Answer 1

Answer:

162.35 amu

Explanation:

Let A represent isotope X-159

Let B represent isotope X-163

Let C represent isotope X-164

The following data were obtained from the question:

Isotope >>> Abundance >>> Mass no

A >>>>>>>> 30.60 >>>>>>>> 159.37

B >>>>>>>> 15.79 >>>>>>>>> 162.79

C >>>>>>>> 53.61 >>>>>>>>> 163.92

Average Atomic mass =.?

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

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

= [(159.37 × 30.60)/100] + [(162.79 × 15.79)/100] + [(163.92 × 53.61)/100]

= 48.77 + 25.70 + 87.88

= 162.35 amu

Therefore, the average atomic mass of element X is 162.35 amu