The average atomic mass of element X is 10.81 u.
The average atomic mass of X is the weighted average of the atomic masses of its isotopes.
We multiply the atomic mass of each isotope by a number representing its relative importance (i.e., its % abundance).
Thus,
0.199 × 10.013 u = 1.993 u
0.801 × 11.009 u = 8.818 u
TOTAL = 10.81 u
Answer:
[tex]m=10.811 amu[/tex]
Explanation:
The average atomic mass in amu is calculated using the following formula
[tex]m=\frac{(m_{1} \%m_{1})+(m_{2} \%m_{2})}{100 \%}[/tex]
[tex]m_{1}= 10.013\\ \%m_{1}= 19.9\%(abundance)\\ m_{2}= 11.009\\ \%m_{2}= 80.1\%(abundance)[/tex]
[tex]m=\frac{((10.013).(19.9\%))+((11.009) (80.1\%))}{100 \%}\\ m=10.811 amu[/tex]
