Answer: The average atomic mass of this element is 131.5 amu
Explanation:
Mass of isotope 1 = 131.90 amu
% abundance of isotope 1 = 90% = [tex]\frac{90}{100}=0.9[/tex]
Mass of isotope 2 = 127.90 amu
% abundance of isotope 2 = 10% = [tex]\frac{10}{100}=0.1[/tex]
Formula used for average atomic mass of an element :
[tex]\text{ Average atomic mass of an element}=\sum(\text{atomic mass of an isotopes}\times {{\text { fractional abundance}})[/tex]
[tex]A=\sum[(131.90\times 0.9)+(127.90\times 0.1)]=131.5amu[/tex]
The average atomic mass of this element is 131.5 amu
The average atomic mass of this element is 131.5 amu
Since Mass of isotope 1 = 131.90 amu
So percentage abundance of isotope should be 90% or 0.9
And, the Mass of isotope 2 = 127.90 amu
So, percentage abundance of isotope 2 = 10% = 0.10
Now the average atomic mass should be
= (90% of 131.90) + (10% of 127.90)
= 131.50
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