Respuesta :
Answer:
69.726 amu
Explanation:
From the question given above, the following data were obtained:
Isotope A:
Mass of A = 68.926 amu
Abundance of A (A%) = 60.00%
Isotope B:
Mass of B = 70.925 amu
Abundance of B (B%) = 40.00%
Average atomic mass =?
The average atomic mass of the element can be obtained as shown below:
Average atomic mass
= [(Mass of A × A%)/100] + [(Mass of B × B%)/100]
= [(68.926 × 60)/100] + [(70.925 × 40)/100]
= 41.3556 + 28.37
= 69.726 amu
Therefore, the average atomic mass of the element is 69.726 amu
The average atomic mass of the element is equal to 69.7256 amu.
Explanation:
Given:
An unknown element with two isotopes.
The atomic mass of isotope-1 = 68.926 amu
The percent abundance of isotope-1 = 60.00%
The atomic mass of isotope-2 = 70.925 amu
The percent abundance of isotope-2 = 40.00%
To find:
The average atomic mass of the element.
Solution:
The atomic mass of isotope-1 = 68.926 amu
The percent abundance of isotope-1 = 60.00%
The fractional abundance of isotope-1 = 0.6000
The atomic mass of isotope-2 = 70.925 amu
The percent abundance of isotope-2 = 40.00%
The fractional abundance of isotope-2 = 0.4000
The average atomic mass of an element = A
[tex]A=\sum [{\text{Atomic mass of an isotope}\times \text{Fractional abundance of an isotope}}]\\A=68.926 amu\times 0.6000+70.925 amu\times 0.4000\\A=69.7256 amu[/tex]
The average atomic mass of the element is equal to 69.7256 amu.
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